In the reaction of 2.75 g of magnesium metal with excess hydrochloric acid, what volume of hydrogen gas will be produced by the reaction if the lab occurs at 25.0oC and 765 torr? (Hint: write a balanced chemical reaction first and do stoichiometry, then use the ideal gas law)
What pressure will be exerted by 45.0 grams of CO2 at a temperature of 25 ˚C and a volume of 630. mL
In the reaction of 2.75 g of magnesium metal with excess hydrochloric acid, what volume of hydrogen gas will be produced by the reaction if the lab occurs at 25.0oC and 765 torr? (Hint: write a balanced chemical reaction first and do stoichiometry, then use the ideal gas law)
Step 1. Write and balance the equation.
Mg + 2HCl ==> MgCl2 + H2
Step 2. Convert g Mg to mols Mg = 2.75 g/atomic mass Mg = ?
Step 3. Convert mols Mg to mols H2 produced using the coefficients in the balanced equation. ?mols Mg from step 2 x (1 mols H2/1 mol Mg) = ?
Then use PV = nRT and plug mols Mg in for n. Solve for V in L. Remember to use T in kelvin. If you use R as 0.08206 then convert pressure to atm.
Post your work if you get stuck.
What pressure will be exerted by 45.0 grams of CO2 at a temperature of 25 ˚C and a volume of 630. mL
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Use PV = nRT.
You will need to convert grams to mols. n = grams/molar mass = ?
Again remember to use T in kelvin. Post your work if you get stuck.
To find the volume of hydrogen gas produced in this reaction, we need to follow a few steps:
Step 1: Write the balanced chemical equation for the reaction between magnesium and hydrochloric acid:
Mg + 2HCl -> MgCl2 + H2
Step 2: Calculate the number of moles of magnesium used. This can be done using the molar mass of magnesium:
Number of moles = mass of magnesium / molar mass of magnesium
Molar mass of magnesium = 24.31 g/mol
Number of moles of magnesium = 2.75 g / 24.31 g/mol = 0.113 mol
Step 3: Determine the stoichiometry of the reaction. From the balanced equation, we can see that 1 mole of magnesium produces 1 mole of hydrogen gas.
Step 4: Use the ideal gas law to calculate the volume of hydrogen gas.
The ideal gas law equation is:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
In this case, we are given the pressure in torr, so we need to convert it to atmospheres and the temperature from Celsius to Kelvin.
Temperature in Kelvin = (25.0 + 273.15) K = 298.15 K
Pressure in atmospheres = 765 torr / 760 torr/atm = 1.007 atm
Now we can plug our values into the ideal gas law equation:
(1.007 atm)(V) = (0.113 mol)(0.0821 L·atm/mol·K)(298.15 K)
Step 5: Solve for the volume of hydrogen gas:
V = (0.113 mol)(0.0821 L·atm/mol·K)(298.15 K) / (1.007 atm)
V = 2.17 L
So, the volume of hydrogen gas produced in the reaction is 2.17 liters.