Answer:
40.02 calories
Explanation:
V = 10 mL = 10g
we know t went <em>up</em> by 4°C, this is our ∆t as it is a change.
Formula that ties it together: Q = mc∆t
where,
Q = energy absorbed by water
m = mass of water
c = specific heat of water (constant)
∆t = temperature change
Q = (10 g) x (4.186 J/g•°C) x (4°C)
Q = 167.44 J
Joules to Calories:
167.44 J x 1 cal/4.184 J = 40.02 calories
(makes sense as in image it is close to the value).
Answer:
111 L
Explanation:
Calculation of moles of hydrogen gas:-
Mass of = 18.6 g
Molar mass of = 2.01588 g/mol
According to the given reaction:-
2 moles of hydrogen gas on reaction produces one mole of acetic acid gas.
So,
1 mole of hydrogen gas on reaction produces mole of acetic acid gas.
Also,
9.23 mole of hydrogen gas on reaction produces mole of acetic acid gas.
Moles of acetic acid gas = 4.615 moles
Given that:
Temperature = 35 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (35 + 273.15) K = 308.15 K
n = 4.615 moles
P = 1.05 atm
V = ?
Using ideal gas equation as:
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L atm/ K mol
Applying the equation as:
1.05 atm × V = 4.615 moles ×0.0821 L atm/ K mol × 308.15 K
<u>⇒V = 111 L</u>
pH of the solution is calculated using the following formula:
Here, is concentration of hydrogen ion.
Initial value of pH is 6.7, calculate concentration of hydrogen ion from this as follows:
Putting the value,
Thus, initial concentration of hydrogen ion is .
Now, final pH value is 8.7, calculate concentration of hydrogen ion as follows:
Thus, final concentration of hydrogen ion is .
The ratio of final to initial value will be:
Thus, if pH increases from 6.7 to 8.7, concentration of hydrogen ion becomes of the initial value.