Search: demonstrate o2 product of reaction

Number of results: 21,456

Chemistry
Consider the reaction, CH4(g) + 2 O2(g) => CO2(g) + 2 H2O(g). How many grams of H2O(g) will be made by the reaction of 17 moles of CH4(g) with 7 moles of O2(g)?
Monday, November 29, 2010 at 11:41pm by Alle

chemistry
Get a second opinion on this AND check my thinking.. N2O5 ==> N2O3 + O2 N2O3 ==> N2O + O2 Add the two equations to obtain N2O5 ==> N2O + 2O2 and k for this reaction is k1*k2 = 7.75*4 = 31.0 = (N2O)(O2)/(N2O5). The final O2 is 4.5 moles; some came from ...
Saturday, February 12, 2011 at 10:55pm by DrBob222

Chemistry 12
Is O2(g) <---> O2(aq) an endothermic/exothermic reaction, and why?
Wednesday, May 4, 2011 at 8:14pm by JM

chemistry
Consider the following reaction. 4Fe + 3O2=2Fe2O3 a. How many moles of O2 are required to react completely with 29.8 mg of Fe? 4.00 x 10^-4 moles O2 b. How many grams Fe2O3, are produced from the complete reaction of 17.8 g of Fe? 25.4 g Fe2O3
Tuesday, February 14, 2012 at 10:29pm by krystal

chemistry
.0815 moles NO are reacted with .0789moles O2 gas to form NO2 gas according to the following equation: 2NO +O2=2NO2 determine the molar amounts of NO, O2 and NO2 after complete reaction.
Tuesday, September 14, 2010 at 10:34pm by Missy

chemistry
One thing that you should note quickly is that the equilibrium constant expression depends on how we write the chemical reaction. For example, consider the following reaction N2O5(g) < - > 2NO2(g) + 1/2O2(g) K = [NO2]2[O2]1/2/[N2O5] However, we can just as easily...
Sunday, July 22, 2012 at 7:14pm by bobpursley

chemistry
The heat for the equation you wrote is 286 kJ/mol of product formed (which I found in a table) and since there are two moles of product, then 286 x 2 = 572 kJ for the reaction as written (to include the 2 moles). So as written the heat emitted is 572 kJ. Why the key wants to ...
Monday, May 18, 2009 at 5:06pm by DrBob222

Economics
3. Suppose a firm has a constant marginal cost of $10. The current price of the product is $25, and at that price, it is estimated that the price elasticity of demand is -3.0. a. Is the charging the optimal price for the product? Demonstrate how you know. b. Should the price ...
Monday, September 3, 2012 at 1:19am by Michelle

chemistry
In a system at equilibrium, the PRODUCT of the concentrations of the products of the reaction divided by the PRODUCT of the reactants, each raised to a power indicated by the coefficient in the balanced chemical equation, is a constant. In orther words, take the products of ...
Monday, August 4, 2008 at 6:11pm by DrBob222

Chemistry
Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) ¨ 2NO2(g) Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and ...
Sunday, October 31, 2010 at 9:32pm by Sarah

Chemistry
Given the following data, calculate the enthalpy change for the reaction S(s)+ O2(g)->SO2(g) S(s)+(3/2)O2(g)->SO3(g) H=-395.2 kJ 2SO2(g)+ O2(g)->2SO3(g) H=-198.2 kJ
Tuesday, January 10, 2012 at 11:10pm by Alisa

chemistry
it depends on the reaction, can you type the reaction equation? for the Le Chatelier's principle you need to know the whole reaction, not just the product
Tuesday, January 27, 2009 at 6:59pm by Anonymous

Solubility of gases
I used to use the handbook of chemistry and physics "Rubber book" for this sort of problem, I presume there must be one available on-line or you could check you college library. So for the gases above CO2 is partially soluble in water but can be collected by downward...
Tuesday, November 15, 2011 at 2:13am by Dr Russ

Organic Chem
A LITTLE CONFUSED...QUESTION ASKS THE REAGENT SHOWN IS ADDED TO THE COMPOUND, WHAT SHOULD YOU SEE WHEN THE TWO MATERIALS ARE MIXED TOGETHER? IS THE ANSWER THE PRODUCT OR THE REACTION, LIKE HEAT OR COLOR CHANGE. AND IF ITS PRODUCT IM CONFUSED? PLEASE HELP. 1.CH3-CH=CH-CH3 + ...
Wednesday, January 17, 2007 at 7:59pm by Desiree

Chemistry
2 H2O (l) → 2 H2 (g) + O2 (g) Using the thermodynamic values to calculate accurate values of ΔHr and ΔSr, will the reaction be product favored at high temperature? Why? Thank you
Friday, November 5, 2010 at 9:03pm by John

Chemistry
In a combination reaction, 2.22 g of Magnesium is heated with 3.75 g of Nitrogen a) which reactant is present in excess? b) how many moles of product are formed? c) after reaction, how many grams of each reactant and product are present?
Monday, October 10, 2011 at 3:35pm by Saige

Chemistry
The reaction written correctly is: 2NiO (s)--> 2Ni(s) + O2 (g) 1. Divide 25.67g NiO by the formula its mass to get the number of moles of NiO. 2. Since 2 moles NiO produce 1 mole O2, moles of O2 = ( ___mol NiO)(1/2) 3. Look up the vapor pressure of water, P(vapor), at ...
Monday, December 7, 2009 at 7:39pm by GK

s.t mary's school
You are talking about two separate reactions. Oxygen (O2) is being made with the reaction 2 KClO3 -> 2 KCl + 3 O2 while H2 is (we will assume) being made with the reaction Zn + 2 HCl -> ZnCl2 + H2 First, convert 30 g of KClO3 to moles. One mole of potassium ...
Thursday, August 9, 2012 at 3:06am by drwls

Chemistry
Step reactions Given: H2O2(l) –> H2O(l) + 1/2 O2(g) ∆H = -98.0 kJ 2 H2(g) + O2(g) –> 2 H2O(l) ∆H = -571.6 kJ Reverse the first reaction and change the sign of the ∆H. Divide all the coefficients of the 2nd reaction and the...
Saturday, October 18, 2008 at 10:36pm by GK

Chemistry
This is a limiting reagent problem. How do I know that. Because BOTH reactants are given. Basically, what we do is work two simple stoichiometry problems, identify the limiting reagent as the one producing the smaller amount of product. CH4(g) + 2 O2(g) => CO2(g) + 2 ...
Monday, November 29, 2010 at 11:41pm by DrBob222

ap chemistry
Calculate the standard reaction enthalpy for the reaction NO2(g) ! NO(g) + O(g) Given: O2(g) ! 2O(g) H = +498.4 kJ/mol NO(g) + O3(g) ! NO2(g) + O2(g) H = −200 kJ/mol 3O2(g) ! 2O3(g) H = +285.4 kJ/mol
Wednesday, October 31, 2012 at 5:40pm by cheri

CHEmistry
The balanced reaction equation for combustion of Mg is: 2 Mg + O2 --> 2 MgO. In the reaction vessel you have 1.0 moles of Mg and 0.30 moles of O2. What is the limiting reactant? How many moles of MgO can you possibley make?
Sunday, October 9, 2011 at 10:07pm by Amanda

college chem
At 750°C, the Kp for the reaction 2 CO + O2➞ 2 CO2 is 2.72 x 10^11. ( 2.72 times ten to the eleventh) At that temperature, CO and O2 are added to a constant volume vessel. The initial pressure of the CO is 2.00 atm, and that of the O2 is 1.50 atm. Calculate the ...
Saturday, February 27, 2010 at 8:16pm by josh

Chemistry
In an experiment, 0.0300 moles each of SO3(g), S02(g), and O2(g) were placed in a 10.0L flask at a certain temperature. When the reaction came to equilibrium, the cocentration of SO2(g) in the flask was 3.50x10^-5 molar. What is Kc for the reaction? 2SO2(g) + O2(g) <--&...
Monday, November 19, 2012 at 1:44am by Mitch

managerial economicsQ4
Consider a Cournot duopoly, composed of firms A & B ¡V which produce identical products and face identical costs. (a) Draw a set of reaction functions in one diagram for this Cournot duopoly. (b) Label the monopoly outputs that would be produced by firms A & B. (...
Sunday, September 7, 2008 at 11:06pm by jenny

Chemistry
I'm not sure I would call that a dissociation reaction. When I think of a dissociation reaction the AgCl ==>? Ag^+ + Cl^- is one; another one is CH3COOH ==> H^+ +CH3COO^-, NaCl + H2O => Na^+(aq) + Cl^-(aq), etc. What you have written I call a reaction...
Thursday, March 8, 2012 at 10:34pm by DrBob222

AP Biology
After an enzyme is mixed with its substrate, the amount of product formed is determined at 10-sec intervals for 1 min. Data: 0 secs. = 0.0 product formed (mg) 10 secs = .25 product formed (mg) 20 secs = .50 product formed (mg) 30 secs = .70 product formed (mg) 40 secs = .80 ...
Sunday, October 7, 2007 at 1:01pm by Mon

Chemistry
The Kc for the reaction below is 4.8 X 10 ^-10. 1/2 N2 +1/2 O2 = NO what is the Kc for the following reaction? 2NO=N2 +O2
Monday, November 1, 2010 at 10:48pm by Missy

Chemistry
Did I do these right? Can someone let me know if I did them correctly? I had someone help me with the problems but know I want to make sure their the right answers? 1. Methane burns in oxygen according to the following equation: CH4 + 2O2 ----> CO2 + 2H2O What is the ...
Tuesday, September 8, 2009 at 4:22pm by Jessie T

Chemistry 11
Which is reactant and product ? 1) C(s)+O2(g)--> CO2 (g) 2) N2(g)+ O2(g) --> 2NO(g)
Saturday, September 11, 2010 at 8:41pm by Anonymous

Chemistry (Stoichiometry)
what mass of so2 is produced from the reaction between 31.5g of s8 and 8.65g of o2? I know how to find the limiting reagents and all but I need a little help knowing how to find the mass of the product.
Monday, May 3, 2010 at 2:09pm by Jill

? on Chemistry
For what it's worth, this is what I think. But I will rewrite the equation. 2N2 + O2 + heat ==> 2NO2 Adding NO2 will force the reaction to the left. I think the intent of the question is to answer that NO2 will decrease because the reaction shifts to the left (but ...
Friday, February 19, 2010 at 8:54pm by DrBob222

Chemistry(Please respond, thank you)
Step 1:H2O2 + I^-^ = H2O + OI^-^ step 2: H2O2 + OI^-^ = H2O + O2 + I^-^ What is the equation for the overall reaction? I am not sure how to do this since there are two equations. Which species acts as a catalyst? I know that I^-^ is the catalsyt. Which species acts as a ...
Wednesday, April 18, 2012 at 5:18pm by Hannah

Chemistry(Thank you for your help)
Step 1:H2O2 + I^-^ = H2O + OI^-^ step 2: H2O2 + OI^-^ = H2O + O2 + I^-^ What is the equation for the overall reaction? I am not sure how to do this since there are two equations. Which species acts as a catalyst? I know that I^-^ is the catalsyt. Which species acts as a ...
Tuesday, April 17, 2012 at 2:14pm by Hannah

Chemistry
2 CO (g) + O2 (g) --> 2 CO2 (g) The mechanism below has been proposed for this reaction; (slow) O2 + CO --> CO2 + O (fast) O + CO --> CO2 Based on this mechanism what is the rate law for this reaction?
Thursday, February 10, 2011 at 8:43pm by John

Chemistry
2 CO (g) + O2 (g) --> 2 CO2 (g) The mechanism below has been proposed for this reaction; (slow) O2 + CO --> CO2 + O(fast) O + CO --> CO2 Based on this mechanism what is the rate law for this reaction?
Tuesday, February 8, 2011 at 1:26pm by John

Chemistry
Calculate the enthalpy change for the reaction: 2S(s) + 3O2(g) --> 2SO3(g) Use the following thermochemical equations: Reaction S(s) + O2(g) --> SO2(g) Delta H(in kJ) -296.8 2SO2(g) + O2(g) --> 2SO3(g) Delta H(in kJ) -197.0
Wednesday, October 13, 2010 at 8:06pm by Jordin

Chemistry
Just a note to clarify a couple of points. #1. IF S were the product, and probably it is not, you would write it as S8. SO2 is the more likely product. #2. I notice you went through mols. When all of the products are gases, you can use a short cut and not go through mols. The ...
Thursday, December 13, 2007 at 9:40pm by DrBob222

chemistry
Determine Kc at 298 K for the reaction 2 CH4(g) reverse reaction arrow C2H2(g) + 3 H2(g), given the following data at 298 K. (Hint: How are Kc and Kp for the reaction related?) CH4(g) + H2O(g) reverse reaction arrow CO(g) + 3 H2(g) Kp = 1.2 multiplied by 10-25 2 C2H2(g) + 3 O2...
Wednesday, March 24, 2010 at 6:21pm by Jenny

chemistry-help!
The initial rate of reaction for H2O2(aq) <-> H2O (l) 1/2 O2 (g) is found to be 1.7x10(-3)M/s. Assume that this rate holds for 2 minutes. Start with 160ml of 1.60 M H2O2. How many milliliters of O2 measured at 24C and 760mmHg , are released from solution in the ...
Monday, November 21, 2011 at 4:04pm by Matt

chem
2H202--> 2H20 +O2 Given that you started with ½ cup of H2O2, what was the mass of each product in the reaction? (1/2 cup = 118.3 mL, density of H2O2 is 1.4 g/mL)
Tuesday, February 12, 2008 at 3:09pm by john

chem
1.05 g of O2 is 1.05/32 = 0.0328125 moles 1.22 g of H2 is 1.22/2.016 = 0.60516 moles O2 is the limiting reactant. There is more than enough H2 to combine with the available oxygen. Each mole of O2 forms 2 moles of H2O, according to the reaction 2H2 = O2 -> 2H2O ...
Sunday, March 9, 2008 at 4:10pm by drwls

chem
Predict the direction of the net reaction in each of the following system, as a result of increasing the temperature. Delta H is an indicator or whether the reaction releases heat delta H(-), or heat is absorb delta H(+). Write where the direction shifts. a)3O2(g)=2O3(g) H=+...
Wednesday, November 28, 2012 at 11:32pm by Angel Locsin

Chemistry(Please help, thank you!)
Using this data, 2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10-3 NO2(g) == NO(g) + ½ O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g) I do not understnad how I am suppose to use the Kc values given if ...
Wednesday, March 14, 2012 at 9:04pm by Hannah

Chemistry
For the reaction system, 2 H2O(g) + O2(g) == 2 H2O2 (g), the equilibrium concentrations are (H2O2) = 0.120 M; (H2O) = 0.860 M; (O2) = 0.330 M. Calculate the value of Kc for this reaction. A. 0.423 B. 0.872 C. 0.0590 D. 1.31 E. 2.51 I did 0.120 / 0.860 X 0.330 = 4.4228 = 4.23...
Saturday, March 3, 2012 at 10:25pm by Hannah

chemistry
1 mole of CS2 = 12.011 + 32.066x2 = 76.143 g/mol (50.92 g) / (76.143 g/mol) = 0.66874 moles CS2 Based on the chemical equation DrBob gave you for the combustion of CS2, (0.66874 mol CS2)(3 mol O2 / 1 mol CS2) = ___moles O2 To get the mass (grams) of O2 consumed in the reaction...
Tuesday, June 24, 2008 at 8:35pm by Anonymous

Chemistry
consider the reaction: N2(g) + O2 (g) --> 2NO (g) removing some of the N2(g) will_____ A) increase the concentration of O2 B) decrease the concentration of O2 C) increase the concentration of NO(g)
Friday, April 20, 2012 at 9:46pm by Shannon

chemistry
figure how many moles of Sb is one gram. Then, you need 1/2 that number of moles of Sb2O4. That is the number of moles of Sb2O4 in the first reaction. Then you need 5 times that number of moles of O2. putting it together, you figure the moles of Sb. Then you need 5/2 of that ...
Wednesday, January 25, 2012 at 12:19pm by bobpursley

Chemistry
What is the standard enthalpy of reaction for the following reaction: H2 + 1/2 O2 --> H2O(g)
Friday, March 11, 2011 at 4:59pm by Lauren

someone correct my work please? fun, fun chemistry
Okay. I'm very, very confused. The initial question is: predict the products of the electrolysis of a 1 mol/L solution sodium chloride. This is my work: The four different possible equations are: 2H2o + 2e- -------> H2 + 2OH- (V= -0.83) O2 + 4H+ + 4e- -------&gt...
Tuesday, January 30, 2007 at 11:31am by Rienna

Chemistry
That makes sense because in this SN1 reaction a E1 reaction competes with the carbocation intermediate and forms a side product...which is 2-methyl-2-butene. But I don't understand why or why not the fraction is included in the product. Is it just because their boiling ...
Thursday, March 19, 2009 at 5:35pm by Sara

college chemistry
Which of the following terms would be in the product(s) for the correctly balanced equation if the equilibrium expression is: [CO2]2/[CO]2[O2] a. O2 b. 2 CO2 c. CO2 d. 2 CO
Thursday, November 4, 2010 at 10:43pm by barbra

ap chemistry
Nitroglycerin is a shock-sensitive liquid that detonates by the reaction 4C3H5(NO3)3(`) −! 6N2(g) + 10H2O(g) + 12CO2(g) + O2(g) Calculate the total volume of product gases at 210 kPa and 296C from the detonation of 2.7 lb (1224.7 g) of nitroglycerin. Answer in ...
Saturday, February 9, 2013 at 7:52pm by cheri

Chem.
The equation tells us (if the reaction goes to completion) that 1 mol O2 produces 2 mols SO3. Those are the coefficients in the balanced equation. Therefore, 12 L SO3 x (1 mol O2/2 mol SO3) = 6 L O2.
Thursday, December 11, 2008 at 12:23am by DrBob222

Chemistry
thank you. I don't understand why the O2 is to the power of two in the rate = k[NO][O2]2 when that is only a first order reaction and the NO is second order.
Tuesday, March 27, 2012 at 5:16am by ll

chemistry
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 NO(g) + O2(g) → 2 NO2(g), ΔH°rxn = ? Given: N2(g) + O2(g) → 2 NO(g), ΔH°rxn = +183 kJ 1/2 N2(g) + O2(g) → NO2...
Tuesday, June 14, 2011 at 10:37pm by Amber

Chemistry
Use oxidation numbers to identify reaction is REDOX reactions. a. 2SO2(g) + O2(g) -> 2SO2(g) for 2SO2 I got: -2 for S, -2 for O for O2 I got 0 for 2SO2 I got -2 for S again, and -2 again for 0 Therefore I lost one oxygen and a REDOX reaction occured Am I right?????
Sunday, June 19, 2011 at 2:11pm by Amy

chemistry
You find n from the mass of oxygen (O2) n = (100.0 g of O2) / (1 mol O2 /32.00 g O2) =3.1 mol of O2 1 mol of any gas at STP has a volume of 22.4 L 1 mole of O2 = 32.0 g of O2 1 mole of O2 = 22.4 L of O2 100.0 g of O2 / 32.00 g of O2 = 3.1 mol of O2 3.1 mol of O2 * 22.4 L/ mol...
Friday, September 25, 2009 at 4:35am by me

Chemistry
Write a balanced equation for the overall reaction: Step 1 O3 + Cl --> O2 + ClO Step 2 ClO + O --> Cl + O2 = O3 + O --> 2O2 Is that correct? or would it be O3 + O --> O2 + O2
Sunday, February 10, 2008 at 11:37pm by Anonymous

CHEM
How many liters of O2 will react with 100 liters of H2 according to the gas phase reaction: O2 + 2H2 ------2H2O
Friday, May 3, 2013 at 6:30pm by MICHELLE

apchemistry
The numerical value of the concentration equilibrium constant for the gaseous reaction 2 SO2 + O2 *) 2 SO3 is 0.5 at temperature T. When a reactionmix- ture is brought to equilibrium, [O2] is found to be 2.0 M and [SO3] is found to be 10 M. What is the equilibrium ...
Wednesday, January 30, 2013 at 5:52pm by cheri

Chemistry 105
Consider the following chemical reaction. 2H2O(l) -->2H2(g)+O2(g) What mass of H2O is required to form 1.6 L of O2 at a temperature of 330 K and a pressure of 0.954 atm?
Sunday, October 23, 2011 at 5:48pm by JULIE

chemistry
1. Write and balance the equation. 2a. mols O2 = grams/molar mass 2b. mols CH4 = grams/molar mass. 3a. Convert mols O2 to mols of a product. 3b. Do the same for mols CH4. 3c. The limiting reagent in these problems is ALWAYS the reagent that provides the FEWER mols product.
Tuesday, January 22, 2013 at 12:45am by DrBob222

Organic Chemistry
The purpose of adding concentrated H2SO4 to the Diels-Alder adduct was to: A. hydrolyze the product to make the product precipitate more easily B. catalyze the diels alder reaction C. use Le Chatelier’s principle to drive the reaction to completion D. to quench excess ...
Friday, March 6, 2009 at 5:18am by nilee

Chem Class
The equilibrium constant for reaction 1 is K.....? how do i figure out problems like this? do i check which ones cancel out? The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ___? (1) SO2 (g) + (1/2) O2 (g) (right and left arrows)SO3 (g...
Monday, October 25, 2010 at 6:59pm by Awr

CHEMISTRY
In each reaction, calculate the moles of product (in parentheses) when 3.00 moles of each reactant is used. A: 4Li+O2 = 2Li2O (Li2O) B: Fe2O3+3H2 = 2Fe+3H2O (Fe) C: Al2S3+6H2O = 2Al(OH)3+3H2S (H2S) Please show work, Thanks
Wednesday, October 31, 2012 at 1:48pm by Boo Boo

chemistry
For each reaction, calculate the moles of product (in parentheses) when 2.00 moles of each reactant is used A: 2SO2 + O2 = 2SO3 (SO3) B: 3Fe + 4H2O = Fe3O4 + 4H2 (Fe3O4) C: C7H16 + 11O2 = 7CO2 + 8H2O (CO2)
Wednesday, October 31, 2012 at 8:17pm by Boo Boo

chemistry
2H2 (g) O2 (g) --> 2H2O (g) if 44 g of O2 are reacted , determine the amount if heat transferred in the reaction when the Heat = -483.6 kJ
Monday, December 12, 2011 at 12:44am by becca

Chemistry 130
Will someone help me by letting me know if I did these correct, or if there the correct answers? Thanks! 2 (10). If two moles of hydrogen gas (H2) react in the following equation, how many moles of H2O will be formed? 2H2 + O2 „³ 2H2O a. 2 moles b. 4 moles c. 1 mole ...
Tuesday, September 8, 2009 at 1:27pm by Jessie

ap chem
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen and methane: 2NH3(g) + 3O2(g) + 2CH4 -->2HCN + 6H2O(g) a)If 5.00 x 10^3 kg each of NH3 , O2, and CH4 are reacted what mass of HCN will be produced, assuming 100% yield? b)At the end ...
Monday, October 11, 2010 at 9:11pm by Emma

Chemistry
OK. You didn't say it this way but I THINK, from the wording in the problem, that you have 5.00 mols Li and 5.00 mols O2 (those are the reactants) and you want to know how much Li2O (the indicated product) is formed. To convert mols of one thing to mols of another, you use...
Monday, May 7, 2012 at 11:32pm by DrBob222

Chemistry
Given the following data: S(s) + 3/2 O2(g)-->SO3(g) ∆H = -395.2 kJ 2SO2(g) + O2(g) -->2SO3(g)∆H = -198.2 kJ Calculate ∆H for the reaction S(s) + O2(g) --> SO2(g) Could someone please tell me how you would go about doing this ...
Tuesday, January 22, 2013 at 6:40pm by Eddie

Chem
Which of the following is the formation reaction for CaO(s) ? A. CaO(s) Ca(s) + 21O2(g) B. Ca2+(aq) + O2–(aq) CaO(s) C. 2 Ca(s) + O2(g) 2CaO(s) D. Ca(s) + 21O2(g) CaO(s). E. 2 CaO(s) 2 Ca(s) + O2(g) I know that you have to create an equation and I believe that the CaO is...
Sunday, February 24, 2008 at 8:16pm by Anonymous

10th grade Chemistry
I don't know if they react with all elements the same. I do know that Pb(NO3)2 reacts with BOTH Na2CrO4 and Na2Cr2O7 to produce the same product of PbCrO4. CrO4^-2 is the product in basic solution and Cr2O7^-2 is the product in acid solution. The two are shown below as a ...
Thursday, January 27, 2011 at 10:45pm by DrBob222

Chemistry
In the reaction 2H20(aq) --> O2(g) + 2H20(l) why doesn't increasing the pressure of oxygen have any effect on the reaction rate? Balance the equation first. What you have isn't balanced. Frankly, it doesn't look possible. You have two mols H2O on each side. ...
Thursday, April 19, 2007 at 6:45am by Fiona

Physics
it is more definitive than this. c is perpendicular to the plane a and b lie in. you have to start with the definition of cross product i x j=k j x k=i k x i=j if a= a1 i + a2 j +a3 k and if b= b1 i + b2 j +b3 k then you can demonstrate with algebra (do it longhand) that a x b...
Wednesday, November 16, 2011 at 10:52am by bobpursley

Chem
I'm baffled. Mg + O2 ==> MgO which is a synthesis reaction. How you can get a decomposition, sr or dr out of that one reaction I don't know.
Tuesday, November 25, 2008 at 8:42pm by DrBob222

Chemistry
Hi can someone please help with this question, or atlest direct me in the right direction. Please and thank you. The initial rate of reaction H2O2(aq) --> H2O (l) + 1/2 O2(g) is found to be1.7*10^-3 M/s . Assume that this rate holds for 2 minutes. Start with 165ml of 1....
Thursday, November 20, 2008 at 3:08am by Melanie

chemistry urgent
Balance the equation. Note the coefficents on Fe and O2, that is the mole ratio. calcuate how many moles of Fe, and O2 you have. Which is the limiting reactant. For instance, if the coefficents were 45Fe+ 34O2, the mole ratio of O2 to Fe is 34/45 If you had 2.3 moles of Fe, ...
Tuesday, November 30, 2010 at 4:14pm by bobpursley

Chemistry
Consider the following chemical equation. SO2(g) + O2(g) → SO3(g) What volume of sulfur dioxide gas reacts with 37.5 L of O2? The reaction conditions are 875°C and 1.00 atm pressure.
Sunday, December 5, 2010 at 10:36pm by Kalen

Chemistry
In this reaction, 4.58 L of O2 were formed at 745mm Hg and 308 K. How many grams of Ag2O decomposed. 2 Ag2O----> 4 Ag + O2 Please help I'm very confused
Monday, October 17, 2011 at 2:14pm by Monique

chemistry
Usually it gives the copper(I) oxide. 4Cu + O2 ==>2Cu2O but to balance the equation for which you asked it is 2Cu + O2 ==> 2CuO It is a synthesis reaction.
Thursday, January 22, 2009 at 5:33pm by DrBob222

chemistry
K= [NO2]^2/([NO2]^2 * [O2]) conc NO2= sqrt(K*NO^2 * O2) = sqrt(1.71E12*.0048^2*.000057) = sqrt( 2250) moles/liter check my work, it is easy to make a math error typo on a keyboard. This is based on the very high forward reaction K you gave. I dont remember this reaction being ...
Monday, September 12, 2011 at 6:30pm by bobpursley

Science
Find the reaction quotient or Q. Q = (SO2)^2 x (O2)/(SO3)^2 Q = (0.480)^2(0.561)/(0.220)^2 Q = 2.67 Compare this to K = 0.23 in the problem. Q is to high meaning SO2 and O2 are too high and SO3 is too low; therefore, it much shift to the left to reach equilibrium. That way SO2...
Thursday, June 30, 2011 at 11:15pm by DrBob222

equilibrium question
For the reaction N2(g)+o2(g)<-->2NO(g), you have the initial concentration [N2]=0.03 and [O2]=0.08 Keq for the reaction at this temperature is 5.7*10^-5. What are the equilibrium concentrations for N2, O2, and NO? Please help me with this! http://www2.ucdsb.on.ca...
Friday, April 13, 2007 at 2:23pm by Chrissy

chemistry
Start from the equation for the reaction O2 + 2H2 -> 2H2O so 1 mole of O2 reacts with 2 moles of H2. 75 g of H2 gas contains 75 g/2 g mole^-1 = 37.5 mole this will react with 37.5 mole/2 moles of O2 (from the equation) hence calculate the number of grams of O2 gas (...
Thursday, January 13, 2011 at 2:52am by Dr Russ

Chemistry
All volume measurements are carried out at the same temperature and pressure. If 20.0 L of O2 (g) are allowed to completely react with a sample of pure CH4 (g) in a combustion process producing CO2 (g) as the only carbon-containing product, what is the maximum volume of CH4 (g...
Thursday, December 1, 2011 at 4:58pm by Anonymous

integrated science
Carbon is a solid. The other two are gasses. You breathe oxygen (O2) in and CO2 out. In combustion, O2 is a reactant and CO2 is a product. That should get you started. Do your own research. It isn't that hard in the internet age
Monday, February 7, 2011 at 4:07pm by drwls

physics
Refering to reaction 2 H2(g) + O2(g) -> 2 H2O(g) and proving that the law of conservation of mass is obeyed during a chemical reaction.
Friday, March 2, 2012 at 3:44am by Belly.L

chemistry
Explain the reaction mechanism of the following reaction by showing the types of bond splitting and atom rearrangements. C + O2 = CO2
Sunday, November 20, 2011 at 10:55pm by Elijah Bowie

Chemistry
Explain the reaction mechanism of the following reaction by showing the types of bond splitting and atom rearrangements. C + O2 = CO2
Sunday, November 20, 2011 at 10:53pm by Elijah Bowie

Chemistry
Given the balanced equation representing a reaction: 2CO(g)+O2(g)-->2CO2(g) what is the mole ration of CO(g) to CO2(g)in this reaction? (1)1:1 (2)1:2 (3)2:1 (4)3:2
Sunday, January 2, 2011 at 8:40pm by lisa fortuna

chemistry
Write the equation. Use PV = nRT and solve for n, the number of mols O2. Convert mols O2 to grams O2, then %O2 = (g O2/g solution)*100 = ?? check my thinking.
Thursday, February 7, 2008 at 8:15pm by drbob222

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