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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:action containing solid copper(I) and oxygen gas combines to form copper(I) oxide. How mañy
Suns or product are produced if you start with 4.00 g of solid copper(I) and 1.25 g of oxygen gas?
Cu(s) + O2(g)
→ Cu,O(s)
A: 4.51 g
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- -W (8a): If 35.92 g CH4 and 70.86 g 0₂ combust, how many grams of CO2 are produced? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H₂O (g)arrow_forwardbIron metal reacts with chlorine gas giving iron(III) chloride. The balanced chemical equation for this reaction is: 2 Fe(s) + 3 Cl₂ (g) → 2 FeCl3 (s) Beginning with 32.0 g of iron, what mass of Cl2, in grams, is required for complete reaction? Mass = g Cl₂ What mass of FeCl3 can be produced? g FeCl₂ Mass=arrow_forwardA website promoting the use of alternative energy vehicles and hybrid technologies claims that "A typical automobile in the USA uses about 500 gal of gasoline every year, producing about 5 tons of carbon dioxide." To determine the truth of this statement, calculate how many tons of carbon dioxide are produced when 500.0 gal of gasoline are combusted. Assume that the primary ingredient in gasoline is octane, C H₁ (1), which has a density of 0.703 g · mL-¹. 18 CO₂ produced: tonsarrow_forward
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- Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/molarrow_forwardAn ore sample is known to contain copper sulfate pentahydrate, CuSO4•5H2O. If a 10.392 g sample of the ore loses 0.9630 g of water when heated strongly, what is the maximum mass, in grams, of CuSO4•5H2O that could have been in the sample? (MW of CuSO4•5H2O = 249.55 g/mol)arrow_forwardChromium metal can be produced from high-temperature reactions of chromium (III) oxide with liquid silicon. The products of this reaction are chromium metal and silicon dioxide. If 8.21 grams of chromium (III) oxide and 4.11 grams of Si are combined, determine the total mass of reactants that are left over.arrow_forward
- d Iron metal reacts with chlorine gas giving iron (III) chloride. The balanced chemical equation for this reaction is: 2 Fe(s) + 3 Cl₂ (g) → 2 FeCl3 (s) If 32.0 g each of iron and chlorine are combined, what is the theoretical yield of iron (III) chloride? 9 Submitarrow_forwardConsider the reaction of solid P₄ and chlorine gas to form gaseous phosphorus trichloride. The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). How many grams of phosphorus trichloride can be formed from 419.7 grams of P₄ based on the balanced chemical equation?arrow_forward
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