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Shtirlitz [24]
3 years ago
12

What mass of water is required to react completely with 157.35 g CO2? (Molar mass of H2O = 18.02 g/mol; molar mass of CO2 = 44.0

1 g/mol
Chemistry
1 answer:
svlad2 [7]3 years ago
6 0

Answer: the answer is 49.05

Explanation:

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Answer:

Knowing this, researchers from the University of Southern Denmark decided to investigate the size of these hypothetical hidden particles. According to the team, dark matter could weigh more than 10 billion billion (10^9) times more than a proton.

Explanation:

If this is true, a single dark matter particle could weigh about 1 microgram, which is about one-third the mass of a human cell (a typical human cell weighs about 3.5 micrograms), and right under the threshold for a particle to become a black hole.

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What is the chemical formula of the following compound
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A. C3H10 is the answer
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2 years ago
Which choice is not an example of a molecule? OF O H202 O 03 O NC13​
MissTica

Answer:

Think it's NC13

Explanation:

It's the only one missing in the molecule

5 0
3 years ago
A 0.885 M solution of KBr whose initial volume is 82.5 mL has more water added until its concentration is 0.500 M. What is the n
4vir4ik [10]

Answer:

V_2=146mL

Explanation:

Hello there!

In this case, since the equation for the calculation of dilutions is:

M_1V_1=M_2V_2

Whereas M is the molarity and V the volume, because the final concentration is lower than the initial. Thus, since we are asked to calculate the final volume, we solve for V2 as follows:

V_2=\frac{M_1V_1}{M_2}=\frac{0.885M*82.5mL}{0.500M}\\\\V_2=146mL

Best regards!

4 0
2 years ago
An air compressor draws in 1,200 cf of free air at a gauge pressure of 0 psi and a temperature of 70°F. The air is compressed to
lubasha [3.4K]

Answer:

The final volume of air after compression: V₂ = 4477.63 L = 158.12 cf

Explanation:

Given: Initial gauge pressure of the gas = 0 psi

Initial absolute pressure of the gas: P₁ = gauge pressure + atmospheric pressure = 0 psi + 12.20 psi = 12.20 psi

Initial Temperature = 70°F

⇒ T₁ = (70°F − 32) × 5/9 + 273.15 = 294.26 K

Initial volume of the gas: V₁ = 1200 cf = 1200 × 28.317  = 33980.4 L    (∵ 1 cf ≈ 28.317  L)

Final gauge pressure of the gas = 90 psi

Final absolute pressure of the gas: P₂ = gauge pressure + atmospheric pressure = 90 psi + 12.20 psi = 102.2 psi

Final Temperature: T₂ = 125°F

⇒ T₂ = (125°F − 32) × 5/9 + 273.15 = 324.82 K

Final volume of the gas: V₂ = ? L      

<u>According to the </u><u>Combined gas law</u><u>:</u>

\frac{P_{1}\times V_{1}}{T_{1}} = \frac{P_{2}\times V_{2}}{T_{2}}

→ V_{2} = \frac{P_{1}\times V_{1}\times T_{2}}{T_{1}\times P_{2}}

→ V_{2} = \frac{12.20 psi\times 33980.4 L\times 324.82 K}{294.26 K\times 102.2 psi}

→ V_{2} = 4477.63 L = 158.12 cf

<u>Therefore, the final volume of air after compression: </u><u>V₂ = 4477.63 L = 158.12 cf</u>

7 0
3 years ago
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