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In the following chemical reaction: 2H,(g) + 0,(g) → 2H,O(g) 1.1 How many moles of H,0 will be produced from 6 moles of 0.? 1.2 How many moles of H, will react with 40 g of 0.? 1.3 How many grams of H,O will be produced by 18 g of H,? itrate solution i

In the following chemical reaction: 2H,(g) + 0,(g) → 2H,O(g) 1.1 How many moles of H,0 will be produced from 6 moles of 0.? 1.2 How many moles of H, will react with 40 g of 0.? 1.3 How many grams of H,O will be produced by 18 g of H,? itrate solution i

Chemistry
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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Worked example 3 Determine the mass of oxygen (0,) consumed in the reaction from Worked example 2 on page 205. Step 1 Write a balanced equation 2H,(g) + 0,(g) → 2H,0(g) Step 2 Write down the 2 moles + 1 mole - 2 moles mole'ratio for the equation Step 3 Calculate molar M (O,) = [(2 x 16)] = 32 g.mol M„(H,) = [(1 x 2)] = 2 g.mol m(H,) is 8,00 g, so number of moles of H, is: masses Step 4 Calculate number of moles 8,00 g = 2 g.mol- = 4 moles Step 5 Write down the 2 moles H, reacts with 1 mole O,, therefore: moles in the moles H, reacts with 2 moles O, reaction Mass of O, consumed: m =n x M = 2,00 mol x 32 g.mol- = 64 g 64 g of oxygen is consumed. Step 6 Determine the mass of the product(s) Step 7 Conclusion Activity 1 Perform stoichiometric calculations In the following chemical reaction: 2H,(g) + O,(g) → 2H,O(g) 1.1 How many moles of H,0 will be produced from 6 moles of O,? 1.2 How many moles of H, will'react with 40 g of 0,? 1.3 How many grams of H,O will be produced by 18 g of H,? Zinc metal is used to displace silver from a silver nitrate solution in accordance with the following equation: Zn(s) + 2AGNO, (aq) – Zn(NO,), (aq) + 2Ag(s) What mass of zinc should be used to displace 60 g of silver from excess silver nitrate solution? 80 g of magnesium react with oxygen in accordance with the reaction equation: 2Mg + 0,- 2MGO. What mass of magnesium oxide is formed? 4 If 33 g of hydrogen was produced when some aluminium was dissolved in hydrochloric acid, what mass of aluminium was dissolved? The balanced equation is: 2A1(s) + 6HCI(aq) → 2AICI, (aq) + 3H,(g) What is the mass of two moles of potassium dichromate (K,Cr0,)? 6. nerical 2 2,5 moles; 18 g. 3 133 g: 5 Calculate the number of moles represented by 9,85 x 10-g of gold (Au). lule 6 Chemical change (Part 2)
Transcribed Image Text:Worked example 3 Determine the mass of oxygen (0,) consumed in the reaction from Worked example 2 on page 205. Step 1 Write a balanced equation 2H,(g) + 0,(g) → 2H,0(g) Step 2 Write down the 2 moles + 1 mole - 2 moles mole'ratio for the equation Step 3 Calculate molar M (O,) = [(2 x 16)] = 32 g.mol M„(H,) = [(1 x 2)] = 2 g.mol m(H,) is 8,00 g, so number of moles of H, is: masses Step 4 Calculate number of moles 8,00 g = 2 g.mol- = 4 moles Step 5 Write down the 2 moles H, reacts with 1 mole O,, therefore: moles in the moles H, reacts with 2 moles O, reaction Mass of O, consumed: m =n x M = 2,00 mol x 32 g.mol- = 64 g 64 g of oxygen is consumed. Step 6 Determine the mass of the product(s) Step 7 Conclusion Activity 1 Perform stoichiometric calculations In the following chemical reaction: 2H,(g) + O,(g) → 2H,O(g) 1.1 How many moles of H,0 will be produced from 6 moles of O,? 1.2 How many moles of H, will'react with 40 g of 0,? 1.3 How many grams of H,O will be produced by 18 g of H,? Zinc metal is used to displace silver from a silver nitrate solution in accordance with the following equation: Zn(s) + 2AGNO, (aq) – Zn(NO,), (aq) + 2Ag(s) What mass of zinc should be used to displace 60 g of silver from excess silver nitrate solution? 80 g of magnesium react with oxygen in accordance with the reaction equation: 2Mg + 0,- 2MGO. What mass of magnesium oxide is formed? 4 If 33 g of hydrogen was produced when some aluminium was dissolved in hydrochloric acid, what mass of aluminium was dissolved? The balanced equation is: 2A1(s) + 6HCI(aq) → 2AICI, (aq) + 3H,(g) What is the mass of two moles of potassium dichromate (K,Cr0,)? 6. nerical 2 2,5 moles; 18 g. 3 133 g: 5 Calculate the number of moles represented by 9,85 x 10-g of gold (Au). lule 6 Chemical change (Part 2)
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