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Gas Stoichiometry Scenario #3 What mass (in grams) of sodium chloride (NaCl) will be produced when enough sodium (Na) is combined with 2.4 L of chlorine gas (Cl₂) at 25 C and 1.2 atm? Na + Cl₂ ⇒ NaCl 2. Check for STP. 1. Check for a balanced chemical equation. If it's not balanced, balance it. This is important for mole ratio if you'll need it. . R = gas constant 8.31 L kPa/mole * K 0.0821 L atm/mole * K PV = nRT 3. Are you given liters or grams? If there's not STP (0 C, 1 atm), you'll need to use Ideal Gas Law to find "V" or "n". If you're given liters, change to moles using the Ideal Gas Law. Once you have moles, you can use mole ratio and molar mass stoichiometry to determine a mass for the product. If you're given grams, change to moles using molar mass and apply a mole ratio to determine "n" for the other chemical. Once you have "n" for the other chemical, you can use the Ideal Gas Law to solve for "V".

Gas Stoichiometry Scenario #3 What mass (in grams) of sodium chloride (NaCl) will be produced when enough sodium (Na) is combined with 2.4 L of chlorine gas (Cl₂) at 25 C and 1.2 atm? Na + Cl₂ ⇒ NaCl 2. Check for STP. 1. Check for a balanced chemical equation. If it's not balanced, balance it. This is important for mole ratio if you'll need it. . R = gas constant 8.31 L kPa/mole * K 0.0821 L atm/mole * K PV = nRT 3. Are you given liters or grams? If there's not STP (0 C, 1 atm), you'll need to use Ideal Gas Law to find "V" or "n". If you're given liters, change to moles using the Ideal Gas Law. Once you have moles, you can use mole ratio and molar mass stoichiometry to determine a mass for the product. If you're given grams, change to moles using molar mass and apply a mole ratio to determine "n" for the other chemical. Once you have "n" for the other chemical, you can use the Ideal Gas Law to solve for "V".

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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Gas Stoichiometry Soenario #3 What mass (in grams) of sodium chloride (NaCl) will be produced when enough sodium (Na) is combined with 2.4 L of chlorine gas (Cl₂) at 25 C and 1.2 atm? Na + Cl₂ ⇒ NaCl 1. Check for a balanced chemical equation. . 2. Check for STP. If it's not balanced, balance it. This is important for mole ratio if you'll need it. R = gas constant 8.31 L kPa/mole * K 0.0821 L* atm/mole * K 3. Are you given liters or grams? PV = nRT If there's not STP (0 C, 1 atm), you'll need to use Ideal Gas Law to find "V" or "n". . If you're given liters, change to moles using the Ideal Gas Law. Once you have moles, you can use mole ratio and molar mass stoichiometry to determine a mass for the product. If you're given grams, change to moles using molar mass and apply a mole ratio to determine "n" for the other chemical. Once you have "n" for the other chemical, you can use the Ideal Gas Law to solve for "V"."
Transcribed Image Text:Gas Stoichiometry Soenario #3 What mass (in grams) of sodium chloride (NaCl) will be produced when enough sodium (Na) is combined with 2.4 L of chlorine gas (Cl₂) at 25 C and 1.2 atm? Na + Cl₂ ⇒ NaCl 1. Check for a balanced chemical equation. . 2. Check for STP. If it's not balanced, balance it. This is important for mole ratio if you'll need it. R = gas constant 8.31 L kPa/mole * K 0.0821 L* atm/mole * K 3. Are you given liters or grams? PV = nRT If there's not STP (0 C, 1 atm), you'll need to use Ideal Gas Law to find "V" or "n". . If you're given liters, change to moles using the Ideal Gas Law. Once you have moles, you can use mole ratio and molar mass stoichiometry to determine a mass for the product. If you're given grams, change to moles using molar mass and apply a mole ratio to determine "n" for the other chemical. Once you have "n" for the other chemical, you can use the Ideal Gas Law to solve for "V"."
Gas Laws Ideal Gas Law If you have 4 moles of gas at a pressure of 5.6 atm and a volume of 12 L, what is the temperature of that gas in Kelvin? P = 5.6 atm V = 12 L n = 4 mol R = 0.0821 Latm/mole*k T= 5.6 atm*12, 4 mol*0.0821/ atm/mole K Solve the following 67.2/0.3284= 1. 2. = 205 K 3. 4. 5. Identify givens and the unknown. Convert all temperatures to Kelvin. Rearrange the equation if you'd like. Substitute values into the equation. Solve for the unknown. PV = nRT R-gas constant 8.311 kPa/mole K 0.0821 Latm/mole K problems: If you have 7.7 moles of gas at a pressure of 0.09 atm and a temperature of 56 °C, what is the volume of the container? 0.09 atm P = 0.09 atm 7.7 mol*0.0821 L atm/mole K*329 K V= n = 7.7 mol R = 0.0821 atm/mole k T= 56 C=56+273=329 207.98393/0.09 2311 L
Transcribed Image Text:Gas Laws Ideal Gas Law If you have 4 moles of gas at a pressure of 5.6 atm and a volume of 12 L, what is the temperature of that gas in Kelvin? P = 5.6 atm V = 12 L n = 4 mol R = 0.0821 Latm/mole*k T= 5.6 atm*12, 4 mol*0.0821/ atm/mole K Solve the following 67.2/0.3284= 1. 2. = 205 K 3. 4. 5. Identify givens and the unknown. Convert all temperatures to Kelvin. Rearrange the equation if you'd like. Substitute values into the equation. Solve for the unknown. PV = nRT R-gas constant 8.311 kPa/mole K 0.0821 Latm/mole K problems: If you have 7.7 moles of gas at a pressure of 0.09 atm and a temperature of 56 °C, what is the volume of the container? 0.09 atm P = 0.09 atm 7.7 mol*0.0821 L atm/mole K*329 K V= n = 7.7 mol R = 0.0821 atm/mole k T= 56 C=56+273=329 207.98393/0.09 2311 L
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