The equivalent volume of hydrogen at STP from one gram of a divalent metal when treated with a
dilute mineral acid is 560 ml, calculate the atomic mass of metal
with an explanation
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The equivalent volume of hydrogen at STP from one gram of a divalent metal when treated with a
dilute mineral acid is 560 ml, calculate the atomic mass of metal
with an explanation
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Answer:
40 grams
Explanation:
Let us first see the chemical reaction between dilute acid and the divalent metal
M+ 2H+=H2 + M2+
From the above equation we can see that 1 mole of divalent metal liberates 1 mole of H2.
Now first let us calculate moles of H2 in 560ml or 0.560L of H2 gas.
Given density of H2 gas is 0.08988 g/L
Mass = Density x volume
Mass = 0.0503 gram
Number of moles = mass / molar mass
Number of moles = 0.0503 / 2 = 0.025
Now 0.025 moles of H2 means we had 0.025 moles of metal
0.025 = 1 / molar mass
Molar mass = 1/0.025 = 40 g