Answer:
The state of matter is liquid
Explanation:
Since the frozen point in celcius is 32 then at 30 its still liquid
The Ksp refers to the equilibrium constant for a solid dissolving in an aqueous solution.
Ksp= 5.61×10⁻¹¹
The equation for this reaction is:
Mg(OH)₂ (s) ⇔ Mg²⁺ (aq) + 2 OH⁻ (aq)
And the associated equilibrium expression is:
Ksp = [Mg2+] x [OH–]²
Mg(OH)₂ its solid and because of that doesn't have molarity, so its not included.
Ksp = [Mg²⁺] x [OH–]²
5.61x10⁻¹¹ = (x) (0.200)²
x = 1,4025 x 10⁻⁹
Since the question manages to include moles, pressure, volume, and temperature, then it is evident that in order to find the answer we will have to use the Ideal Gas Equation: PV = nRT (where P = pressure; V = volume; n = number of moles; R = the Universal Constant [0.082 L·atm/mol·K]; and temperature.
First, in order to work out the questions, there is a need to convert the volume to Litres and the temperature to Kelvin based on the equation:
250 mL = 0.250 L
58 °C = 331 K
Also, based on the equation P = nRT ÷ V
⇒ P = (2.48 mol)(0.082 L · atm/mol · K)(331 K) ÷ 0.250 L
⇒ P = (67.31 L · atm) ÷ 0.250 L
⇒ P = 269.25 atm
Thus the pressure exerted by the gas in the container is 269.25 atm.
Answer:
1.2 g
Explanation:
<u>For gallium:-</u>
Mass of gallium= 4.00 g
Molar mass gallium = 69.723 g/mol
The formula for the calculation of moles is shown below:
Thus,
<u>For arsenic:-</u>
Mass of arsenic = 5.50 g
Molar mass of arsenic = 74.9216 g/mol
The formula for the calculation of moles is shown below:
Thus,
According to the given reaction:
1 mole of gallium react with 1 mole of Arsenic
0.0574 mole of gallium react with 0.0574 mole of Arsenic
Moles of arsenic required = 0.0574 moles
Available moles of arsenic = 0.0734 moles
Limiting reagent is the one which is present in small amount. Thus, gallium is limiting reagent.
Moles left unreacted of arsenic = 0.0734 moles - 0.0574 moles = 0.016 moles
<u>Mass = Moles * Molar mass = 0.016 * 74.9216 g = 1.2 g</u>