Question

Consider the following reaction: 2 NH3 (g) + 3 Cl2 (g) ? N2 (g) + 6 HCl (g) A mixture is prepared from 15.0 mol of ammonia and 15.0 mol of chlorine gas. Determine the total moles of gas in the container after the reaction has gone to completion. Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal place. Answer: In an experiment, the decomposition of hydrogen peroxide, H2O2 (aq), was used to produce oxygen gas, O2 (g). 2 H2O2 (aq) ? 2 H2O (l) + O2 (g) The reaction flask contained the H2O2 and the test tube inside the flask contained a catalyst to speed up the reaction. The volume of oxygen gas produced was determined by water displacement. To determine the moles of oxygen produced, the reaction flask, including its contents, was weighed before and after the reaction. During the reaction the flask was placed in a cold water bath to cool the solution. After the reaction, if the outside of the reaction flask was still wet when it was weighed, how would this affect the molar volume of the oxygen gas that was determined? Select one: A. This would not significantly affect the molar volume of the gas. B. The molar volume of the oxygen gas determined would be too small. C. The molar volume of the oxygen gas determined would be too large. D. More information is needed to answer this question.

          Consider the following reaction:
2 NH3 (g) + 3 Cl2 (g) ? N2 (g) + 6 HCl (g)
A mixture is prepared from 15.0 mol of ammonia and 15.0 mol of chlorine gas. Determine the total moles of gas in the container after the reaction has gone to completion.
Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal place.
Answer:
In an experiment, the decomposition of hydrogen peroxide, H2O2 (aq), was used to produce oxygen gas, O2 (g).
2 H2O2 (aq) ? 2 H2O (l) + O2 (g)
The reaction flask contained the H2O2 and the test tube inside the flask contained a catalyst to speed up the reaction. The volume of oxygen gas produced was determined by water displacement. To determine the moles of oxygen produced, the reaction flask, including its contents, was weighed before and after the reaction. During the reaction the flask was placed in a cold water bath to cool the solution. After the reaction, if the outside of the reaction flask was still wet when it was weighed, how would this affect the molar volume of the oxygen gas that was determined?
Select one:
A. This would not significantly affect the molar volume of the gas.
B. The molar volume of the oxygen gas determined would be too small.
C. The molar volume of the oxygen gas determined would be too large.
D. More information is needed to answer this question.

Consider the following reaction:
2 NH3 (g) + 3 Cl2 (g) ? N2 (g) + 6 HCl (g)
A mixture is prepared from 15.0 mol of ammonia and 15.0 mol of chlorine gas. Determine the total moles of gas in the container after the reaction has gone to completion.
Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal place.
Answer:
In an experiment, the decomposition of hydrogen peroxide, H2O2 (aq), was used to produce oxygen gas, O2 (g).
2 H2O2 (aq) ? 2 H2O (l) + O2 (g)
The reaction flask contained the H2O2 and the test tube inside the flask contained a catalyst to speed up the reaction. The volume of oxygen gas produced was determined by water displacement. To determine the moles of oxygen produced, the reaction flask, including its contents, was weighed before and after the reaction. During the reaction the flask was placed in a cold water bath to cool the solution. After the reaction, if the outside of the reaction flask was still wet when it was weighed, how would this affect the molar volume of the oxygen gas that was determined?
Select one:
A. This would not significantly affect the molar volume of the gas.
B. The molar volume of the oxygen gas determined would be too small.
C. The molar volume of the oxygen gas determined would be too large.
D. More information is needed to answer this question.

Added by Robert W.

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