For problems (1-7) use the equation: 3 NaHCO3 + H3PO4 ----> 3 CO₂ + 3 H₂O +Na3PO4 Number of moles of CO2 produced from 5.0 moles of H3PO4. The number of grams of CO₂ formed from 3.0 moles of NaHCO3. The number of grams of NaHCO3 needed to produce 6.80 moles of water. Grams of CO₂ resulting when 49.0 g of H3PO4 reacts. 1. 2. 3. 4. 450 of Na. PO.2
For problems (1-7) use the equation: 3 NaHCO3 + H3PO4 ----> 3 CO₂ + 3 H₂O +Na3PO4 Number of moles of CO2 produced from 5.0 moles of H3PO4. The number of grams of CO₂ formed from 3.0 moles of NaHCO3. The number of grams of NaHCO3 needed to produce 6.80 moles of water. Grams of CO₂ resulting when 49.0 g of H3PO4 reacts. 1. 2. 3. 4. 450 of Na. PO.2
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1,2,3,4 please
![**Practice Assignment: Stoichiometry**
On a separate sheet of paper, show the setup and answer for each problem. Follow the formal problem-solving method that is illustrated in the examples above.
For problems (1-7), use the equation:
\[ 3 \, \text{NaHCO}_3 + \text{H}_3\text{PO}_4 \rightarrow 3 \, \text{CO}_2 + 3 \, \text{H}_2\text{O} + \text{Na}_3\text{PO}_4 \]
1. Number of moles of \( \text{CO}_2 \) produced from 5.0 moles of \( \text{H}_3\text{PO}_4 \).
2. The number of grams of \( \text{CO}_2 \) formed from 3.0 moles of \( \text{NaHCO}_3 \).
3. The number of grams of \( \text{NaHCO}_3 \) needed to produce 6.80 moles of water.
4. Grams of \( \text{CO}_2 \) resulting when 49.0 g of \( \text{H}_3\text{PO}_4 \) reacts.
5. What mass of \( \text{NaHCO}_3 \) reacts in order to produce 450. g of \( \text{Na}_3\text{PO}_4 \)?
6. Calculate the percent yield of \( \text{Na}_3\text{PO}_4 \) if 350. g of \( \text{Na}_3\text{PO}_4 \) are formed from 692 g of \( \text{NaHCO}_3 \).
7. If 100.0 g of \( \text{NaHCO}_3 \) is reacted with 100.0 g of \( \text{H}_3\text{PO}_4 \), which reactant is the limiting reactant?
- Note: \( \text{NaHCO}_3 \) is the limiting reactant (as handwritten on the paper).
For the equation:
\[ \text{H}_2 + \text{CuO} \rightarrow \text{Cu} + \text{H}_2\text{O} \]
8. If 10.0 grams of hydrogen are reacted with \( \text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F89ca33f5-cb99-4448-ba96-35f6ac44a938%2Fceff42c5-f68d-4e49-9a7f-5a71bf0a87d2%2Fmzj37q_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Practice Assignment: Stoichiometry**
On a separate sheet of paper, show the setup and answer for each problem. Follow the formal problem-solving method that is illustrated in the examples above.
For problems (1-7), use the equation:
\[ 3 \, \text{NaHCO}_3 + \text{H}_3\text{PO}_4 \rightarrow 3 \, \text{CO}_2 + 3 \, \text{H}_2\text{O} + \text{Na}_3\text{PO}_4 \]
1. Number of moles of \( \text{CO}_2 \) produced from 5.0 moles of \( \text{H}_3\text{PO}_4 \).
2. The number of grams of \( \text{CO}_2 \) formed from 3.0 moles of \( \text{NaHCO}_3 \).
3. The number of grams of \( \text{NaHCO}_3 \) needed to produce 6.80 moles of water.
4. Grams of \( \text{CO}_2 \) resulting when 49.0 g of \( \text{H}_3\text{PO}_4 \) reacts.
5. What mass of \( \text{NaHCO}_3 \) reacts in order to produce 450. g of \( \text{Na}_3\text{PO}_4 \)?
6. Calculate the percent yield of \( \text{Na}_3\text{PO}_4 \) if 350. g of \( \text{Na}_3\text{PO}_4 \) are formed from 692 g of \( \text{NaHCO}_3 \).
7. If 100.0 g of \( \text{NaHCO}_3 \) is reacted with 100.0 g of \( \text{H}_3\text{PO}_4 \), which reactant is the limiting reactant?
- Note: \( \text{NaHCO}_3 \) is the limiting reactant (as handwritten on the paper).
For the equation:
\[ \text{H}_2 + \text{CuO} \rightarrow \text{Cu} + \text{H}_2\text{O} \]
8. If 10.0 grams of hydrogen are reacted with \( \text
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