Answer:
Explanation:
The pressure is constant, so we can use Charles' Law.
Data:
V₁ = 1.92 × 10³ L; T₁ = 20 °C
V₂ = ?; T₂ = 68 °C
Calculations:
(a) Convert temperatures to kelvins
T₁ = (20 + 273.15) K = 293.15 K
T₂ = (68 + 273.15) K = 341.15 K
(b) Calculate the volume
The new volume of the gas is .
Answer:
Explanation:
Hello!
In this case, considering that the mass of hydrazine is missing, we can assume it is 130.0 g (a problem found on ethernet). In such a way, since we need a mass-mole-atoms relationship by which we can compute moles of hydrazine given its molar mass (32.06 g/mol), then the moles of hydrogen considering one mole of hydrazine has four moles of hydrogen and one mole of hydrogen has 6.022x10²³ atoms (Avogadro's number); therefore, we proceed as shown below:
Notice 130.0 g has four significant figures, therefore the result is displayed with four as well.
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