Reaction between mercury (ii) sulfide with Calcium oxide is as shown;
4 HgS +4 CaO = 4 Hg + 3 CaS + CaSO4
The molar mass of HgS is 232.66 g/mol
The number of moles = 31.28/232.66
= 0.1344 moles
The mole ratio of HgS : CaO is 1: 1
Therefore, the number of moles of Calcium oxide is 0.1344 moles
1 mole of CaO Contains 56 g/mol
Thus, the mass of CaO is 56 g/mol
= 0.1344 moles × 56 g/mol
= 7.5264 g
Your answer would be C because the fire gave the marshmellow a brown crust shwoing effect.
Answer:
0.034 M
Explanation:
1/[A] = kt + 1/[A]o
[A] = ?
k= 0.04556
t= 10.0 minutes or 600 seconds
[A]o = 0.50 M
1/[A] = (0.04556 × 600) + 1/0.50
[A] = 0.034 M
The antacid is alkaline so it neutralizes the excess acids in your stomach.
Answer:
The maximum amount of work that can be done by this system is -2.71 kJ/mol
Explanation:
Maximum amount of work denoted change in gibbs free energy during the reaction.
Equilibrium concentration of B = 0.357 M
So equilibrium concentration of A = (1-0.357) M = 0.643 M
So equilibrium constant at 253 K,
[A] and [B] represent equilibrium concentrations
When concentration of A = 0.867 M then B = (1-0.867) M = 0.133 M
So reaction quotient at this situation,
We know,
where R is gas constant and T is temperature in kelvin
Here R is 8.314 J/(mol.K), T is 253 K, Q is 0.153 and is 0.555
So,
= -2710 J/mol
= -2.71 kJ/mol