Find the mass of one atom of uranium-235. Recall that the mass in atomic mass units is equal to the mass in grams of one mole of
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Answer:
0.591 g of magnesium phosphate is the theoretical yield.
Magnesium nitrate is the limiting reactant.
Explanation:
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In this case, since the balanced reaction turns out:
Next, we compute the grams of magnesium phosphate yielded by each reactant, considering the present mole ratios and molar masses:
Thus, we infer that the correct theoretical yielded mass is 0.591 g as magnesium nitrate is the limiting reactant for which it produces the fewest grams of product.
However, is not possible to compute the percent yield since no actual yield is given, and must be provided or indicated by the problem or an experiment and it not here, nevertheless, you may compute the percent yield by dividing the actual yield by the theoretical and then multiplying by 100:
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<u>Answer:</u> The molar mass of metal is 52.4 g/mol
<u>Explanation:</u>
To calculate the moles of hydrogen gas collected, we use the equation given by ideal gas which follows:
where,
P = pressure of the hydrogen gas = Total pressure - vapor pressure of water = (756.0 - 23.8 ) torr = 732.2 torr
V = Volume of the gas = 201 mL = 0.201 L (Conversion factor: 1 L = 1000 mL)
T = Temperature of the gas =
R = Gas constant =
n = number of moles of hydrogen gas = ?
Putting values in above equation, we get:
The given chemical equation follows:
By Stoichiometry of the reaction:
1 mole of hydrogen gas is formed by 1 mole of metal
So, 0.0083 moles of hydrogen gas will be formed by = of metal
To calculate the molar mass of metal from given number of moles, we use the equation:
Moles of metal = 0.0083 moles
Given mass of metal = 0.435 g
Putting values in above equation, we get:
Hence, the molar mass of metal is 52.4 g/mol