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
d. 8 moles
e. 36 moles
I believe this is a. 2 moles, is that correct?
3 (11). The amount of product that should be produced based on stoichiometric calculations is the¡K.
a. Actual yield
b. Theoretical yield
c. Percent yield
d. Minimum yield
e. Scientific yield
I have b. theoretical yield, is that correct?
4 (12). In an experiment, a laboratory technician produced 4.59 grams of O2 when 4.89 grams of O2 was supposed to be formed based on stoichiometry of the reaction. What was the percent yield for this experiment?
a. -6.1%
b. 106%
c. 93.9%
d. 6.1%
e. 54.3%
I believe this is c. 93.9%, is that right?
5 (13). An alkaseltzer tablet is massed at 3.4 grams. In a beaker, 10.0 grams of water are massed. The tablet and water are carefully placed in a Ziploc bag without mixing and the bag is sealed. The tablet and the water are mixed resulting in fizzing and the bag filling up with gas. What will the total mass in the bag be when the reaction is complete?
a. 3.4 grams
b. 10.0 grams
c. 13.4 grams
d. 6.6 grams
e. More information is needed
I have this one as c. 13.4g, is that correct?
7 (17). Determine the number of moles of MgO that form from the reaction of 4.4 moles of O2 in the following unbalanced equation:
Mg(s) + O2(g) „³ MgO(s)
a. 1.1 moles
b. 4.4 moles
c. 17.6 moles
d. 2.2 moles
e. 8.8 moles
I believe this one is b. 4.4 moles, is that right?
Thank you for the help ;-)
No on 7). Balance the equation.
To determine if your answers are correct, we can go through each question and explain how to solve them.
2 (10). If two moles of hydrogen gas (H2) react in the following equation, how many moles of H2O will be formed?
2H2 + O2 → 2H2O
To find the number of moles of H2O formed, we need to look at the balanced equation. From the equation, we can see that 2 moles of H2 react to form 2 moles of H2O. So, for every 2 moles of H2, we get 2 moles of H2O. Therefore, the correct answer is a. 2 moles.
3 (11). The amount of product that should be produced based on stoichiometric calculations is the…
a. Actual yield
b. Theoretical yield
c. Percent yield
d. Minimum yield
e. Scientific yield
The amount of product that should be produced based on stoichiometric calculations is called the theoretical yield. Theoretical yield represents the maximum amount of product that can be obtained in a reaction assuming complete conversion of reactants to products. Therefore, the correct answer is b. Theoretical yield.
4 (12). In an experiment, a laboratory technician produced 4.59 grams of O2 when 4.89 grams of O2 was supposed to be formed based on stoichiometry of the reaction. What was the percent yield for this experiment?
a. -6.1%
b. 106%
c. 93.9%
d. 6.1%
e. 54.3%
Percent yield is calculated by dividing the actual yield by the theoretical yield, then multiplying by 100%. In this case, the actual yield is given as 4.59 grams and the theoretical yield is given as 4.89 grams. Therefore, the percent yield would be (4.59 / 4.89) * 100% ≈ 93.9%. So, the correct answer is c. 93.9%.
5 (13). An Alka-Seltzer tablet is massed at 3.4 grams. In a beaker, 10.0 grams of water are massed. The tablet and water are carefully placed in a Ziploc bag without mixing, and the bag is sealed. The tablet and the water are mixed, resulting in fizzing and the bag filling up with gas. What will the total mass in the bag be when the reaction is complete?
a. 3.4 grams
b. 10.0 grams
c. 13.4 grams
d. 6.6 grams
e. More information is needed
In this scenario, the reaction between the Alka-Seltzer tablet and water will produce a gas, which will increase the total mass in the bag. Therefore, the total mass in the bag will be more than the sum of the initial masses of the tablet and water. Since there is no information given about the mass of gas produced, the only sensible answer is e. More information is needed.
7 (17). Determine the number of moles of MgO that form from the reaction of 4.4 moles of O2 in the following unbalanced equation:
Mg(s) + O2(g) → MgO(s)
a. 1.1 moles
b. 4.4 moles
c. 17.6 moles
d. 2.2 moles
e. 8.8 moles
To determine the number of moles of MgO formed, we need to determine the stoichiometric ratio between O2 and MgO. From the equation, we can see that the stoichiometric ratio is 1:1, meaning that for every 1 mole of O2, 1 mole of MgO is formed. Therefore, if 4.4 moles of O2 are used in the reaction, the same amount, 4.4 moles of MgO will be formed. So, the correct answer is b. 4.4 moles.
Based on the explanations provided, your answers are all correct except for question 5 (13), where the correct answer is e. More information is needed. Keep up the good work!