Answer:
The mass of ice required to melt to lower the temperature of 353 mL of water from 26 ⁰C to 6 ⁰C is 85.4197 kg
Explanation:
Heat gain by ice = Heat lost by water
Thus,
Heat of fusion + 
Where, negative sign signifies heat loss
Or,
Heat of fusion + 
Heat of fusion = 334 J/g
Heat of fusion of ice with mass x = 334x J/g
For ice:
Mass = x g
Initial temperature = 0 °C
Final temperature = 6 °C
Specific heat of ice = 1.996 J/g°C
For water:
Volume = 353 mL
Density of water = 1.0 g/mL
So, mass of water = 353 g
Initial temperature = 26 °C
Final temperature = 6 °C
Specific heat of water = 4.186 J/g°C
So,
345.976x = 29553.16
x = 85.4197 kg
Thus,
<u>The mass of ice required to melt to lower the temperature of 353 mL of water from 26 ⁰C to 6 ⁰C is 85.4197 kg</u>
The net ionic equation of hydrobromic acid would be HBr = H+ + Br-. As we can see, the HBr compound dissociates into ions where one ion is the hydronium ion which characterizes an acid. According to Arrhenius, an acid is a compound which releases hydronium ion in solution.
Answer: An element os made up of one kind of atom.
Explanation: Dalton's concept states that all atoms of an element is identical.
Answer:
K = [H2] [CO] / [HCHO]
Explanation:
HCHO(g) ⇌ H2(g) + CO(g)
We can obtain the expression for the equilibrium constant for the above equation as follow:
Equilibrium constant, K for a given reaction is the ratio of the concentration of the product raised to their coefficient to the concentration of the reactant raised to their coefficient.
Thus, the equilibrium constant, K for the above equation can be written as follow:
K = [H2] [CO] / [HCHO]
