Answer:
The pressure of a given amount of gas is directly proportional to iys absolute temperature provided that that the volume does not change
Answer:
3.57 g.
Explanation:
- The ratio of cream of tartar (KHC₄H₄O₆) to baking soda (NaHCO₃) in the baking powder is 1:1.
- We need to calculate the number of moles of (8.0 g) of cream of tartar (KHC₄H₄O₆) using the relation:<em> n = mass / molar mass,</em>
mass of cream of tartar (KHC₄H₄O₆) = 8.0 g.
molar mass of cream of tartar (KHC₄H₄O₆) = 188.1772 g/mol.
∴ n of cream of tartar (KHC₄H₄O₆) = mass /molar mass = (8.0 g) / (188.1772 g/mol) = 0.0425 mol.
- Since the mole ratio of the two components is 1:1, the no. of moles of baking soda (NaHCO₃) should be added is 0.0425 mol.
- The quantity of baking soda (NaHCO₃) can be calculated using the relation:
mass = n x molar mass = (0.0425 mol)(84.007 g/mol) = 3.57 g.
Answer:
V ≈ 646.50 L
General Formulas and Concepts:
<u>Chemistry - Gas Laws</u>
- Reading a Periodic Table
- Stoichiometry
- Combined Gas Law: PV = nRT
- R constant - 62.4 (L · torr)/(mol · K)
- Kelvin Conversion: K = °C + 273.15
Explanation:
<u>Step 1: Define</u>
RxN: N₂H₄ (g) + O₂ (g) → N₂ (g) + 2H₂O (l)
Given: 34.9 °C, 755.08 torr, 914.894 g H₂O
<u>Step 2: Identify Conversions</u>
Kelvin Conversion
Molar Mass of H - 1.01 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol
<u>Step 3: Convert</u>
Stoichiometry:
= 25.3955 mol N₂
Temperature: 34.9 + 273.15 = 308.05 K
<u>Step 4: Find Volume</u>
- Substitute variables: (755.08 torr)V = (25.3955 mol)(62.4 (L · torr)/(mol · K))(308.05 K)
- Multiply: (755.08 torr)V = 488160 L · torr
- Isolate <em>V</em>: V = 646.502 L
<u>Step 5: Check</u>
<em>We are given 5 sig figs as our lowest. Follow sig fig rules and round.</em>
646.502 L ≈ 646.50 L
Answer:
24 atm.
Explanation:
From the question given above, the following data were obtained:
Initial volume (V₁) = 240 L
Initial pressure (P₁) = 2 atm
Final volume (V₂) = 20 L
Temperature = constant
Final pressure (P₂) =?
The final pressure required, can be obtained by using the Boyle's law equation as shown below:
P₁V₁ = P₂V₂
2 × 240 = P₂ × 20
480 = P₂ × 20
Divide both side by 20
P₂ = 480 / 20
P₂ = 24 atm
Thus, the final pressure required is 24 atm.
I think it would be these three answers ionic , covalent , and polar covalent