Answer:
1.15 atm
Explanation:
According to Dalton's law of partial pressures, the total pressure is the sum of all the partial pressures of the gases present in the mixture.
Therefore we have:
Total pressure = partial pressure of carbon monoxide + partial pressure of oxygen + partial pressure of carbon dioxide
We were given the following:
Total pressure = 2.45 atm
Pressure of oxygen = 0.65 atm
Pressure of carbon monoxide = x
Pressure of carbon dioxide = 0.65 atm
Therefore:
2.45 = x + 0.65 + 0.65
2.45 = x + 1.3
x = 2.45 - 1.3
x = 1.15 atm
Answer:
rest will do later mom is calling me plz understand promise will do it
Explanation:
- Elements and compounds are similar in that they are both made of atoms and in some cases molecules.
- Methods of Breaking Down Compounds
- The only way to break down a compound is through a chemical change. Sometimes, energy is needed for a chemical change to happen. Two ways to add energy to break down a compound are to apply heat and to apply an electric current.
Net ionic equation
Cu²⁺(aq)+S²⁻(aq)⇒CuS(s)
<h3>Further explanation</h3>
Double-Replacement reactions. Happens if there is an ion exchange between two ion compounds in the reactant to form two new ion compounds in the product
In the ion equation, there is a spectator ion that is the ion which does not react because it is present before and after the reaction
When these ions are removed, the ionic equation is called the net ionic equation
For gases and solids including water (H₂O) can be written as an ionized molecule
Reaction
CuSO₄(aq)+Na₂S(aq)⇒CuS(s)+Na₂SO₄
ionic equation
Cu²⁺(aq)+SO₄²⁻(aq)+2Na⁺(aq)+S²⁻(aq)⇒CuS(s)+2Na⁺(aq+SO₄²⁻(aq)
spectator ions : 2Na⁺ and SO₄²⁻
Net ionic equation
Cu²⁺(aq)+S²⁻(aq)⇒CuS(s)
Answer:
1943.1 moles
Explanation:
From the question given above, the following data were obtained:
Volume (V) = 50200 L
Temperature (T) = 25 °C
Pressure (P) = 720 mmHg
Number of mole (n) of H₂ =?
Next, we shall convert 25 °C to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
Temperature (T) = 25 °C
Temperature (T) = 25 °C + 273
Temperature (T) = 298 K
Next, we shall convert 720 mmHg to atm. This can be obtained as follow:
760 mmHg = 1 atm
Therefore,
720 mmHg = 720 mmHg × 1 atm / 760 mmHg
720 mmHg = 0.947 atm
Thus, 720 mmHg is equivalent to 0.947 atm
Finally, we shall determine number of mole of Hydrogen gas, H₂, needed to fill the balloon as follow:
Volume (V) = 50200 L
Temperature (T) = 298 K
Pressure (P) = 0.947 atm
Gas constant (R) = 0.0821 atm.L/Kmol
Number of mole (n) of H₂ =?
PV = nRT
0.947 × 50200 = n × 0.0821 × 298
47539.4 = n × 24.4658
Divide both side by 24.4658
n = 47539.4 / 24.4658
n = 1943.1 moles
At Equilibrium, The rate of formation of Products is equal to the rate of degradation of Reactants.
Hope this helps!
