The answer is 5.1242x10^8
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
Explanation:
According to the psychrometric chart at dry bulb temperature of and RH 70%, the absolute humidity = 0.011 kg/kg dry air
Formula to calculate humid volume is as follows.
dry air =
=
=
= 0.847 dry air
Hence, humid volume of air is 0.847 dry air.
Specific enthalpy of dry air = specific heat capacity of dry air × dry bulb temperature
=
= 21.126 kJ/kg dry air
Hence, the specific enthalpy of the air is 21.126 kJ/kg dry air.
As per the psychrometric chart at given conditions wet bulb temperature = 17.5
As per the psychrometric chart at given conditions dew point temperature = 15.5
Answer:
1.40 atm
Explanation:
To answer this question we can use<em> Gay-Lussac's law</em>, which states:
When volume and number of moles remain constant.
- T₁ = 23°C ⇒ 23+273.16 = 296.16 K
- T₂ = Boiling point of water = 100 °C ⇒ 100+273.16 = 373.16 K
We <u>put the known data in the equation and solve for P₂</u>:
- 1.11 atm * 373.16 K = P₂ * 296.16 K
Answer:
For me, it is balanced
Explanation:
Because the amount of element Zn reaction is equal the production. Also as the amount of Hydrogen and Chloride in the reaction and the production are equal.