all i really know is that STP (standard temperature and pressure) represents conventional conditions established by IUPAC with T = 273.15 K, P = 1 atm . Now putting these values of temperature and pressure at STP, we can calculate easily volume occupied by 1 mol of gas and which comes out to be 22.4 L. hope this helps
Answer:
Moles = 10.625 mol
Explanation:
Molarity is the amount of solute dissolved per unit volume of solution. It is expressed as,
Molarity = Moles / Volume of Solution ----- (1)
We can also rearrange this equation in terms of moles as,
Moles = Molarity × Volume of Solution ------(2)
Data Given;
Molarity = 4.25 mol.L⁻¹
Volume = 2.50 L
Now, putting value of Molarity and Volume in eq. 2,
Moles = 4.25 mol.L⁻¹ × 2.50 L
Moles = 10.625 mol
Answer:
Which of the following statements about electrical conductors is true?
Right answer gets brainliest
a:They have low resistance.
b:They have high resistance.
c:They control the current.
d:They require high voltage.
I hope its help
Na₂SO₄ → 2Na⁺ + SO₄²⁻
c₁(Na⁺)=2c(Na₂SO₄)
n₁(Na⁺)=c₁(Na⁺)v₁=2c(Na₂SO₄)v₁
NaCl → Na⁺ + Cl⁻
c₂(Na⁺)=c(NaCl)
n₂(Na⁺)=c₂(Na⁺)v₂=c(NaCl)v₂
n(Na⁺)=n₁(Na⁺)+n₂(Na⁺)=2c(Na₂SO₄)v₁+c(NaCl)v₂
v=v₁+v₂
c(Na⁺)=n(Na⁺)/v={2c(Na₂SO₄)v₁+c(NaCl)v₂}/(v₁+v₂)
c(Na⁺)={2*0.400*0.1+0.600*0.2}/(0.1+0.2)=0.667 mol/L
c(Na⁺)=0.667M
Using the Ideal gas law: PV = nRT, where P = pressure, V = volume, n = no. of moles, R= universal gas constant, T = temperature.
Given, n = 0.500 moles, T = 301 K, R=0.0821 L•atm/mol•K, V = 2.5 L
Substituting the given values in the Ideal gas equation:
P = nRT/V = (0.500 mol x 0.0821 L•atm/mol•K x 301 K) / 2.5 L = 4.94 atm
The pressure of carbon dioxide gas = 4.94 atm
