15.63 mol. You need 15.63 mol HgO to produce 250.0 g O_2.
<em>Step 1</em>. Convert <em>grams of O_2 to moles of O_2</em>
Moles of O_2 = 250.0 g O_2 × (1 mol O_2/32.00 g O_2) = 7.8125 mol O_2
<em>Step 2</em>. Use the molar ratio of HgO:O_2 to convert <em>moles of O_2 to moles of HgO
</em>
Moles of HgO = 0.8885 mol O_2 × (2 mol HgO/1 mol O_2) = <em>15.63 mol HgO</em>
Density = mass / volume
= 69g / 23 ml
= 3 g / ml.
Thus, the density of the sample is 3 grams per ml or 3g/ ml
<span>11.2G is the answer to this problem.
</span>
Answer:
13.53 kJ
Explanation:
The energy of a gas can be calculated by the equation:
E = (3/2)*n*R*T
Where n is the number of moles, R is the gas constant (8.314 J/mol.K), and T is the temperature.
E = (3/2)*3.5*8.314*310
E = 13,531.035 J
E = 13.53 kJ
Answer:
Answer in explanation
Explanation:
A. This is wrong. The reactants are on the left side of the yields arrow
B. This is wrong. They can only be at one side at a time. They cannot be on both sides at the same time.
C. The products are on the right side of the yields arrow and not at the left side
D. This is correct. The reactants are on the left side of the yields arrow.
E. This is correct. We can have varying numbers of the number of atoms on both side of the yields arrow. The numbers may differ until we decide to balance the equation