Answer:
5.12 atm
Explanation:
Before you can use the Ideal Gas Law to find the pressure, you need to convert grams to moles (via molar mass).
Molar Mass (H₂): 2(1.008 g/mol)
Molar Mass (H₂): 2.016 g/mol
1.8 grams H₂ 1 mole
---------------------- x ---------------------- = 0.893 moles H₂
2.016 grams
The Ideal Gas Law equation looks like this:
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = Ideal Gas Constant (0.0821 L*atm/mol*K)
-----> T = temperature (K)
After converting Celsius to Kelvin, you can plug the given values into the equation and simplify to find the pressure.
P = ? atm R = 0.0821 L*atm/mol*K
V = 4.3 L T = 27 °C + 273.15 = 300.15 K
n = 0.893 moles
PV = nRT
P(4.3 L) = (0.893 moles)(0.0821 L*atm/mol*K)(300.15 K)
P(4.3 L) = 22.0021
P = 5.12 atm
**Based on my past experiences, I believe the constant (R) you provided may have been mistyped. Instead of 0.821, I used 0.0821.**
Answer:
i think b is the answer hope this helps:))
There are two problems for this question:1. What is the total dollar amount of your profit and loss:
Put option premium is equal to 0.04 per unit.
The exercise price is 1.22
One option contract is 100,000
Selling price is 1.20
-Purchase prise is - 1.22
-Premium paid is +0.04
Net profit is = 0.02 x 100,000 = 2,000 – 80 = 1,920
2. Now undertake that as an alternative of taking a position in the put option one year ago, you sold a future's contract on 100,000 euros with a payment date of one year.
Find the total dollar amount of your profit or loss.
Solution: Contract to buy: $1.20 x 100,000 = 120,000 at payment date.
Contract to sell: $1.22 x 100,000 = 122,000 at settlement date
Settle contracts: -2,000 - 80 = -$2,080
Answer:
See explanation
Explanation:
The equation of the reaction is;
C3H8 + 5O2 ----> 3CO2 + 4H2O
Number of moles of C3H8 = 132.33g/44g/mol = 3 moles
1 mole of C3H8 yields 3 moles of CO2
3 moles of C3H8 yields 3 × 3/1 = 9 moles of CO2
Number of moles of oxygen = 384.00 g/32 g/mol = 12 moles
5 moles of oxygen yields 3 moles of CO2
12 moles of oxygen yields 12 × 3/5 = 7.2 moles of CO2
Hence C3H8 is the limiting reactant.
Mass of CO2 produced = 9 moles of CO2 × 44 g/mol = 396 g of CO2
1 moles of C3H8 yields 4 moles of water
3 moles of C3H8 yields 3 × 4/1 = 12 moles of water
Mass of water = 12 moles of water × 18 g/mol = 216 g of water
b) Actual yield = 269.34 g
Theoretical yield = 396 g
% yield = actual yield/theoretical yield × 100/1
% yield = 269.34 g /396 g × 100
% yield = 68%
<span>The physical layers of the inner core and outer core form a single compositional layer.
</span>
