# How much heat is released when a mixture containing 10.0g CS2 and 10.0 g Cl2 reacts by the equation. CS2 + 3Cl2 ----> S2Cl2 + CCl4 Delta H = -230 kJ

18,767 results
1. ## Chemistry

2H2+O2 -> 2H20 changeHrxn=-484 KJ Which answer best describes the transfer heat that occurs when 1.30 mol of H2 reacts? 629 KJ released 315 KJ absorbed 315 KJ released 484 KJ absorbed 484 KJ released 629 KJ absorbed

2. ## Chemistry

Cl2 reacts with the element Sr to form an ionic compound. Based on periodic properties, identify a molecule, X2, that is likely to to react with Sr in a way similar to how Cl2 reacts with Sr. Justify your choice. *****I think it could be MgCl because Cl2

3. ## chemistry

When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ How many kilojoules are released when 2.65 moles of H2O2 reacts? How many kilojoules are released when 234 g of O2 is produced?

4. ## chemistry

Consider the reaction, C2H4 (g) + H2 (g)- C2H6 (g) where -137kJ of heat is released. How many kilojoules are released when 55.3g of C2H4 reacts?

5. ## chem

At 668K 1 mol each of CO and Cl2 are introduced into an evacuated 1.75 L flask. At equilibrium, the total pressure of the gaseous mixture is 32.4 atm. Calculate Kp. How to solve this ? Co+Cl2CoCl2

6. ## Chemistry

When 0.250 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 177 kJ of heat are released. Calculate the value of Delta H for this reaction, as written. 2CH4(g)+3Cl2(g)-->2CHCl3(l)+3H2(g) delta H=?

7. ## General Chemistry I

When a 0.432g sample of a mixture of volatile hydrocarbons is burned in a bomb calorimeter with heat capacity of 3046 J/C, the temperature rises by 7.82C. How much energy (in KJ) is released during combustion. **I got that answered** 3046x7.82C=23819.72J

8. ## chemistry

at an equilibrium mixture of PCl5, PCl3, and Cl2 has partial pressures of 217.0 Torr, 13.2 Torr and 13.2 Torr respectively. a quantity of Cl2 is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of mixing). the system

9. ## Chemistry

The overall reaction in a commercial heat pack can be represented as shown below. 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) ΔH = -1652 kJ How much heat is released when 4.00 mol iron is reacted with excess O2? How much heat is released when 1.00 mol Fe2O3 is produced?

10. ## chemistry

CH3OH(g) ----> CO(g) + 2H2 (g) (delta H =+90.7k) A) is heat absorbed or released in the course of this reaction? b) calculate the amount of heat transferred when 45.0g of CH3OH(g)is decomposed by this reaction at constant pressure. c) for a given sample of

11. ## chemistry due soon

Which reaction shows that the enthalpy of formation of CS2 is Hf = 89.4 kJ/mol? A. C(s) + 2S(s) CS2(l) + 89.4 kJ B. C(s) + 2S(s) + 89.4 kJ CS2(l) C. C(s) + 2S(s) + 89.4 kJ CS2(l) + 89.4 kJ D. C(s) + 2S(s) CS2(l) I think the answer is a or b

12. ## ap chemistry

How much heat is released if 2.00 moles CF2Cl2 reacts with 70.0 g F2 with a 75.0 percent yield? CF2Cl2 + F2 ! CF4 + Cl2 H for this reaction is -401 kJ/mol rxn. 1. 553 kJ 2. 739 kJ 3. 985 kJ 4. 601 kJ 5. 1069 kJ 6. 802 kJ

13. ## chemistry

When 34.1 g of lead reacts with 6.81 L of oxygen gas, measured at 1.00 atm and 25.0°C, 36.1 kJ of heat is released at constant pressure. What is DH° for this reaction?

14. ## CHEM

2H2+O2=2H2O H=-484KJ Which answer best describes the transfer of heat that occurs when 1.41 mol of H2 reacts with 0.671 mol of O2? 341 kJ released 484 kJ released 341 kJ absorbed 484 kJ absorbed 325 kJ released 325 kJ absorbed

15. ## Chemistry

Consider the following reaction: 2Na + Cl2  2NaCl ΔH = -821.8 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 5.6 g of Na reacts at constant pressure. (c) How many grams of NaCl are produced during an

16. ## Chemistry - Heat of Fusion of Ice

Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the final temperature of the

17. ## Chemistry

In the presence of an alkali, Cl2 reacts to form Cl- and ClO3- , as follows: 3 Cl2(g) + 6 OH−(aq) → 5 Cl−(aq) + ClO3−(aq) + 3 H2O(l) a. Calculate the oxidation number for chlorine in each of the species. b. Write a half equation for the formation

18. ## Chemistry

The value of H° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely.

19. ## chemistry

The value of delata h for the reaction below is -186 kJ. Calculate the heat Kj released from the reaction of 25g of Cl2

20. ## chemistry

How many kilojoules of heat are released when 38.6g of CH4 reacts completely with O2 to form CH3OH at constant pressure?

21. ## chemistry

Phosphorus trichloride gas and chlorine gas reacts to form phosphorus pentachloride gas: PCL3(g) +CL2(g) = PCL5(g). A vessel is CHARGED WITH A MIXTURE OF PCL3(g) and CL2(g), which is allowed to equilibrate at 450K. At equlibrium the partial pressures of

22. ## CHEM

Aluminum reacts with Chlorine gas to form AlCl3. [2Al(s)+3Cl2(g)=2AlCl3(s)] Given 11.0g of Al and 16.0g Cl2, if you had excess Al, how many moles of AlCl3 could be produced from 16.0g of Cl2?

23. ## EPCC

how to calculate the heat (kJ) released to thesurroundings when a 23.0 g of HCL if formed, from a CH4 + Cl2=CHCl3+3HCL

24. ## chemistry(check my answer)

Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction? Cl2(g) + 3F2(g) yield 2ClF3(g) a)-d(Cl2)/dt = -d(F2)/dt b)-d(Cl2)/dt = 2[-d(F2)/dt] c)3[-d(Cl2)/dt] = -d(F2)/dt d)2[-d(Cl2)/dt] =

25. ## Chemistry

How much heat is absorbed/released when 20.00 g of NH2 reacts in the presence of excess O2 to produce NO and H2O according to the following chemical equation: 4NH3 + 5O2 --> 4NO + 6H2O, deltaH= +1168 kJ. The answer is 342.9 kJ of heat absorbed. I want to

26. ## Chemistry

In the following chemical reaction between H2 and Cl2 to produce HCl, what is the mass of HCl produced with 0.35g of H2 completely reacts with 12.42g of Cl2?

27. ## Chemistry

Calculate the heat released when 1.00L of Cl2 (g) with a density of 1.88g/L reacts with an excess of sodium metal at 25 degrees C and 1 atm to form sodium chloride.

28. ## Chemisty

What is the molecularity of each of the following elementary reactions? A. O+O2+N2----> O3+N2+ B. NO2Cl + Cl---> NO2 + Cl2 C. Cl + H2 ---> HCl + H D. CS2----> CS + S

29. ## chemistry

The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s) + O2(g) → 2BaO (s) How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form BaO (s)?

30. ## Chem

Carbon disulfide (CS2) reacts with excess chlorine (Cl2) to produce carbon tetrachloride (CCl4) and disulfur dichloride (S2Cl2). If 67.1 g of CS2 yields 45.2 g of CCl4, what is the percent yield? (Hint, you must first write the balanced equation.) 67.36 I

31. ## chem

How much heat is released if 2.00 moles CF2Cl2 reacts with 70.0 g F2 with a 75.0 percent yield? CF2Cl2 + F2 → CF4 + Cl2 ∆H for this reaction is -401 kJ/mol rxn.

32. ## chemistry

Identify the limiting reagent and the volume of product formed with 11L CS2 reacts with 18L O2 to prduce CO2 gas and SO2 gas. CS2+3O2-->CO2+2SO2

33. ## chemistry

How much heat is released when a mixture containing 12.6 g CS2 and 12.6 g Cl2 reacts by the following equation? CS2(g) + 3 Cl2(g) → S2Cl2(g) + CCl4(g) ΔH° = −230. kJ

34. ## Chem

How much heat is released when a mixture containing 10.0g CS2 and 10.0 g Cl2 reacts by the equation. CS2 + 3Cl2 ----> S2Cl2 + CCl4 Delta H = -230 kJ

35. ## Chemistry

Consider the reaction:P4 (s)+ 6 Cl2 (g) = 4PCl3(g) Delt H = -1230 kJ How much heat is released when 52.5 of Cl2 (g) reacts with an excess of P4 (s)? I tried the question and got -910.8 kJ and the answer is suppose to be -/+ 152 kJ.

36. ## CHEMISTRY

Equilibrium Equation with Partial Pressures PCl3(g) +Cl2(g) PCl5(g)? An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and

37. ## Chemistry

How will the equilibrium: Heat energy + CH4 + 2H2S = CS2 + 4H2 be affected by the following? a) A decrease in temperature? b) The addition of H2 c) The removal of some CH4 d) An increase in the volume of the container e) The addiotion of a catalyst. i know

38. ## Chem 1020

Please help me!!! For the reaction, calculate how many grams of the product form when 3.0 g of Cl2 completely reacts. Assume that there is more than enough of the other reactant. 2Na(s)+Cl2(g)→2NaCl(s)

39. ## chemistry

The dH for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely. 2CO(g) + O2(g) --> 2CO2(g)

40. ## Chemistry

Given the balanced equation: H2 + Cl2 → 2 HCl , how many moles of HCl will be produced if 18.4 g H2 reacts with 127 g Cl2?

41. ## Chemistry

How much heat is released when a mixture containing 12.6 g CS2 and 13.2 g Cl2 reacts by the following equation? CS2(g) + 3 Cl2(g) → S2Cl2(g) + CCl4(g) ΔH° = −230. kJ

42. ## chemistry

How much heat is released when a mixture containing 12.6 g CS2 and 12.6 g Cl2 reacts by the following equation? CS2(g) + 3 Cl2(g) → S2Cl2(g) + CCl4(g) ΔH° = −230. kJ

43. ## chemistry

Calculate the heat released when 3.10 L of Cl2(g) with a density of 1.88 g/L reacts with an excess of sodium metal at 25°C and 1 atm to form sodium chloride. 1 kJ

44. ## Chemistry

Nitrogen monoxide reacts with chlorine gas according to the reaction: 2NO (g) + Cl2 (g) â‡” 2NOCl (g) Kp = 0.27 at 700 K A reaction mixture initially contains equal partial pressures of NO and Cl2 . At equilibrium, the partial pressure of NOCl is 115

45. ## Chemistry

A 10.0 gram sample of a mixture of CH4 and C2H4 reacts with oxygen at 25°C and 1 atm to product carbon dioxide gas and liquid water. If the reaction produces 520 kJ of heat, what is the mass percentage of CH4 in the mixture? PLEASE HELP! I do not know

46. ## Chemistry

A 10.0 gram sample of a mixture of CH4 and C2H4 reacts with oxygen at 25°C and 1 atm to product carbon dioxide gas and liquid water. If the reaction produces 520 kJ of heat, what is the mass percentage of CH4 in the mixture? I am all out of tries on the

47. ## chemistry

The dH for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely. 2CO(g) + O2(g) --> 2CO2(g)

48. ## Chemisty

The value of ∆Ho for the reaction below is -1107 kJ: 2Ba(s) + O2(g) → 2BaO(s) How many kJ of heat are released when 15.75 g of Ba(s) reacts completely with oxygen to form BaO(s)? A) 35.1 B) 114 C) 70.3 D) 20.8 E) 63.5

49. ## Chemistry urgent

2CH3OH(g)→2CH4(g)+O2(g)ΔH=+252.8kJ How many kilojoules of heat are released when 38.8g of CH4(g) reacts completely with O2(g) to form CH3OH(g) at constant pressure?

50. ## chemistry

Solid magnesium metal reacts with chlorine gas according to the following equation: Mg + Cl2 --> MgCl2 What mass of magnesium chloride is formed in the reaction between 7 g of Mg and 13.2 g of Cl2

51. ## Chemistry

How much heat is released when a mixture containing 10.0g CS2 and 10.0 g Cl2 reacts by the equation. CS2 + 3Cl2 ----> S2Cl2 + CCl4 Delta H = -230 kJ

52. ## chemistry

Calculate the heat released when 4.260 L Cl2 with a density of 2.46 g/L at 25°C reacts with an excess of sodium metal to form solid sodium chloride at 25°C.

53. ## Chemistry

Calcium oxide (quicklime) reacts with water to produce calcium hydroxide (slaked lime). CaO(s) + H2O(l) Ca(OH)2(s) ÄH = -65.2 kJ The heat released by this reaction is sufficient to ignite paper. How much heat is released when 29.0 g of calcium oxide

54. ## Chemistry

N2 (g) + 3 CL2 (g) ---> 2 NCL3 (g) delta H = + 230 kj ----- a) What mass of N2 would absorb 96.5 kj of heat as it reacts? b) What volume of Cl2 at STP would be required to react with the N2 in part (a)?

55. ## Chemistry - Heat Calculations

Calculate the heat released when 4 L Cl2 with a density of 2.46 g/L at 25 degrees C reacts with an excess of sodium to form solid sodium chloride at 25 degrees C.

56. ## chemistry

Carbon disulfide (CS2) undergoes a single displacement reaction with O2 to form CO2. If 100 grams of CS2 reacts with 38 grams of O2, what will the limiting reagent be? CS2 + O2 CO2 + 2S carbon disulfide (CS2) carbon dioxide (CO2) oxygen (O2) sulfur (S)

57. ## Chemistry

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has a partial pressure of 217.0 torr, 13.2 torr, and 13.2 torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 torr. The appropriate chemical

58. ## chemistry help

An amount of 414.27 g of zinc sulfide (ZnS, MM=97.44 g/mol) reacts with 99.58 g of oxygen gas (O2, MM=31.999 g/mol) at a constant temperature of 298.0 K and constant pressure of 1.00 atm. The reaction: 2 ZnS(s) + 3 O2(g) --> 2 ZnO(s) + 2 SO2(g) dH =

59. ## chemistry help

An amount of 414.27 g of zinc sulfide (ZnS, MM=97.44 g/mol) reacts with 99.58 g of oxygen gas (O2, MM=31.999 g/mol) at a constant temperature of 298.0 K and constant pressure of 1.00 atm. The reaction: 2 ZnS(s) + 3 O2(g) --> 2 ZnO(s) + 2 SO2(g) dH =

60. ## Chem!!

The value of ƒ¢H‹ for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO(g) reacts completely. 2CO(g) + O2(g) ¨ 2CO2(g)

61. ## Chemistry

What is the molecularity of each of the following elementary reactions? A. O+O2+N2----> O3+N2+ B. NO2Cl + Cl---> NO2 + Cl2 C. Cl + H2 ---> HCl + H D. CS2----> CS + S

The reaction between hydrogen and chlorine gases gives hydrogen chloride gas in the following reaction: H2(g) + Cl2(g) = 2HCl(g) It is found experimentally that 1 mole of H2 gas reacts with 1 mole of Cl2 gas at constant temperature and pressure, to release

63. ## physics

Exactly 11 kJ of energy was absorbed by 1 mol of Cl2(g) at 298 K. What i s thefinal temperature of the Cl2(g)? The heat capacity of Cl2(g) is 25.635J.K-1.mol-1

64. ## science

When you freeze water, 80 calories of heat are released into the surroundings for every gram of water that freezes. This is known as the "latent heat of fusion" of water, which is 80 cal/g. Heat of fusion is a characteristic property. Theoretically, if you

65. ## College Chem

4. Write the balanced equation for CH4+Cl2„_CH2Cl2+HCl6. For the reaction in problem 4, Heat of Reaction = -118.3 kcal/mol. Identify whether this is an exothermic or endothermic reaction. Calculate the Heat of Reaction when 6.00 g of Cl2 are used in the

66. ## chemistry

If 8.29 L of gaseous Cl2 measured at STP and 0.380 mol of liquid CS2 are reacted stoichiometrically according to the balanced equation, how many moles of liquid CS2 remain? CS2(l) + 3Cl2(g) ¡æ CCl4(l) + S2Cl2(l) Molar Mass (g/mol) Cl2 70.906 CS2 76.143

67. ## Chemistry

When i try to do this problem by simply using a mole ratio, wiley keeps saying it's wrong, what mistake am i making? If 0.800 mol of liquid CS2 reacts stoichiometrically according to the balanced equation, how many moles of gaseous Cl2 are required? CS2(l)

68. ## Chemistry

When i try to do this problem by simply using a mole ratio, wiley keeps saying it's wrong, what mistake am i making? If 0.800 mol of liquid CS2 reacts stoichiometrically according to the balanced equation, how many moles of gaseous Cl2 are required? CS2(l)

69. ## Chemistry

The solvent CCl4 is manufactured as follows CS2+Cl2=CCl4+S2Cl2. Balance it and calculate the grams of CS2 needed to react with 62.7 of Cl2?

70. ## Chemistry

Calculate the heat released when 1.61 L of Cl2(g) with a density of 1.88 g/L reacts with an excess of sodium metal at 25°C and 1 atm to form sodium chloride.

71. ## chemistry

Calculate the heat released when 3.10 L of Cl2(g) with a density of 1.88 g/L reacts with an excess of sodium metal at 25°C and 1 atm to form sodium chloride

72. ## chemistry

Calculate the heat released when 4.260 L Cl2 with a density of 2.46 g/L at 25°C reacts with an excess of sodium metal to form solid sodium chloride at 25°C.

73. ## chemistry

When CS2(g) (545.0 grams) and 57.71 grams of H2(g) in a 200.0 L reaction vessel at 961.0 K are allowed to come to equilibrium the mixture contains 2.447 mol of CH4(g). What concentration (mol/L) of CS2(g) reacted? Molar Mass CS2(g) 76.15 H2(g) 2.016 CH4(g)

74. ## Science

Given the following equation: N2 + Cl2 > @ NCL3 H=+230 kJ a) What mass of N2 would absorb 96.5 kJ of heat as it reacts? b) What volume of Cl2 at STP would be required to react with the N2 in part (a)? I do not know how to solve this problem. My mindset is

75. ## Chemistry

How many mL of an impure liquid CS2 mixture (density 1.26 gmL-1) which contains 93.0% of CS2 by mass, must be burned to obtain 12.8g SO2? I cannot get this question! Thanks -D

76. ## Science

Consider the following reaction: 2Na + Cl2  2NaCl ΔH = -821.8 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 5.6 g of Na reacts at constant pressure. (c) How many grams of NaCl are produced during an

77. ## Chemistry

If 49.6 mL of liquid CS2 and 12.8 g of gaseous Cl2 are reacted stoichiometrically according to the balanced equation, how many moles of liquid S2Cl2 are produced? CS2(l) + 3Cl2(g) ¨ CCl4(l) + S2Cl2(l)

78. ## Chemistry

If 61.0 g of gaseous Cl2 and 25.4 mL of liquid CS2 are reacted stoichiometrically according to the balanced equation, how many milliliters of liquid CCl4 are produced? CS2(l) + 3Cl2(g) → CCl4(l) + S2Cl2(l)

79. ## chem

a mixture of 50g of S & 1x10^2g of Cl2 reacts completely to form S2Cl2 &SCl2. Find the mass of S2Cl2 formed.

80. ## chem

a mixture of 50g of S & 1x10^2g of Cl2 reacts completely to form S2Cl2 &SCl2. Find the mass of S2Cl2 formed.

81. ## Chemistry...part 2

Regarding the question I posted earlier (How many mL of an impure liquid CS2 mixture (density 1.26 gmL-1) which contains 93.0% of CS2 by mass, must be burned to obtain 12.8g SO2?)>>volume is 6.49 mL what volume of pure oxygen at 25.0 degrees C and 100 kPa

82. ## Chemistry

If 45.3 mL of liquid CS2 and 7.62 L of gaseous O2 measured at STP are reacted stoichiometrically according to the balanced equation, how many milliliters of liquid CS2 remain? CS2(l) + 3O2(g) -> CO2(g) + 2SO2(g) Molar Mass (g/mol) CS2 76.143 O2 31.998

83. ## chemistry

Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction? Cl2(g) + 3F2(g) yield 2ClF3(g) a)-d(Cl2)/dt = -d(F2)/dt b)-d(Cl2)/dt = 2[-d(F2)/dt] c)3[-d(Cl2)/dt] = -d(F2)/dt d)2[-d(Cl2)/dt] =

84. ## Chemistry12

How will the equilibrium: Heat energy + CH4 + 2H2S = CS2 + 4H2 be affected by the following? a) A decrease in temperature? b) The addition of H2 c) The removal of some CH4 d) An increase in the volume of the container e) The addiotion of a catalyst. i know

85. ## compose

How many kilojoules of heat are released when 25.0 g of {\rm CO}(g) reacts completely with {\rm H_2}(g) to form {\rm CH_3OH}(g) at constant pressure?

86. ## chem

a mixture of 50g of S & 1x10^2g of Cl2 reacts completely to form S2Cl2 &SCl2. Find the mass of S2Cl2 formed. (ans:20.2g) i need the calculation work bcus i got diff. from the ans which is 70.2g.

87. ## chemistry(check my answer)

Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction? a)-d(Cl2)/dt = -d(F2)/dt b)-d(Cl2)/dt = 2[-d(F2)/dt] c)3[-d(Cl2)/dt] = -d(F2)/dt d)2[-d(Cl2)/dt] = -d(F2)/dt e)-d(Cl2)/dt = 3[-d(F2)/dt]

88. ## Chem

The value of ƒ¢H‹ for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO(g) reacts completely. 2CO(g) + O2(g) ¨ 2CO2(g) *I just want to how to solve this problem as in an equation, not the answer.

89. ## Chemistry

When CH4(g) (0.06318 mol/L) and 16.43 mol of H2S(g) in a 130.0 L reaction vessel at 711.0 °C are allowed to come to equilibrium the mixture contains 0.04107 mol/L of CS2(g). What is the equilibrium concentration (mol/L) of H2S(g)? CH4(g)+2H2S(g) =

90. ## chemistry

Solid magnesium metal reacts with chlorine gas according to the following equation: Mg + Cl2 --> MgCl2 What mass of magnesium chloride is formed in the reaction between 7 g of Mg and 13.2 g of Cl2

91. ## chemistry

Solid magnesium metal reacts with chlorine gas according to the following equation: Mg + Cl2 --> MgCl2 What mass of magnesium chloride is formed in the reaction between 7 g of Mg and 13.2 g of Cl2 is this correct 7 g+13.2 g = 20.2 grams ?

92. ## Chemistry

Given the balanced equation: H2 + Cl2 2 HCl , how many moles of HCl will be produced if 18.4 g H2 reacts with 127 g Cl2?

93. ## Chemistry

Is there an equation used to fond remaining pressure When CS2 at partial pressure 1930 torr reacts with H2 at partial pressure 8650 torr at constant volume and constant temperature according to the balanced equation, determine the partial pressure (atm) of

94. ## Chemistry

Is there an equation used to fond remaining pressure When CS2 at partial pressure 1930 torr reacts with H2 at partial pressure 8650 torr at constant volume and constant temperature according to the balanced equation, determine the partial pressure (atm) of

95. ## Chemistry

In the presence of an alkali, Cl2 reacts to form Cl- and ClO3- , as follows: 3 Cl2(g) + 6 OH−(aq) → 5 Cl−(aq) + ClO3−(aq) + 3 H2O(l) a. Calculate the oxidation number for chlorine in each of the species. b. Write a half equation for the formation

96. ## chemistry

at an equilibrium mixture of PCl5, PCl3, and Cl2 has partial pressures of 217.0 Torr, 13.2 Torr and 13.2 Torr respectively. a quantity of Cl2 is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of mixing). the system

97. ## chem

Consider the reaction: CO(g)+Cl2(g)⇌COCl2(g) Keq= 2.9×1010 at 25 ∘C A 5.89 −L flask containing an equilibrium reaction mixture has [CO]= 1.9×10−6 M and [Cl2]= 9.3×10−7 M . How much COCl2 in grams is in the equilibrium mixture?

98. ## chemistry

Solid magnesium metal reacts with chlorine gas according to the following equation: Mg + Cl2 --> MgCl2 What mass of magnesium chloride is formed in the reaction between 7 g of Mg and 13.2 g of Cl2 I got 7/24.3= .288 13.2/70.90= 1.861777 thats as far as i

99. ## chemistry

SiH4(g) + 2 F2(g) SiF4(g) + 4 HF(g) If 18.9 kJ are released when 1.10 g of F2 reacts with an excess of SiH4, what is the heat of the reaction when 1.20 moles of F2 react?

100. ## Chemistry

When deciding upon which fuel source used to power a vechicle, engineers often use the heat released in combustion of differning fuels to make their decision. Would you use the heat released per mole of a hydrocarbon or the heat released per gram of a