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Katena32 [7]
3 years ago
6

When the volume of a gas is changed from mL to 852 mL the temperature will change from 315c to 452c

Chemistry
1 answer:
zhenek [66]3 years ago
4 0

Answer:

The starting volume is 691 mL

Explanation:

The compete question is:

When the volume of a gas is changed from ___ mL to 852 mL, the temperature will change from 315 °C to 452 °C. What is the starting volume?

Write Charles Law and substitute values in:

   V1 / T1 = V2 / T2

    V1 / 588 K = 852 mL / 725 K

   V1 (725 K) = (852 mL) (588 K)

   V1 = 691 mL

Note the large °C values, trying to get you to forget to add 273. Remember, only Kelvin temperatures are allowed in the calculations.

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What acid occurs naturally in the body and performs important regulatory functions
gtnhenbr [62]

Answer: carbonic acid

8 0
3 years ago
Read 2 more answers
Density is the amount of mass per unit volume. Calculate the density of an object that has a mass of 10 Kg and has a volume of 5
Gnoma [55]

Answer: 2 kg/L or 2 g/mL

Explanation:

litres are a cubic measure. “Cubic litres” is redundant at best, potentially confusing.

4 0
2 years ago
1. Methane (CH4) combusts as shown in the equation below. If 3 moles of methane were used in the combustion, what would be the c
umka2103 [35]

Answer:

The change in enthalpy in the combustion of 3 moles of methane = -2406 kJ

Explanation:

<u>Step 1: </u>The balanced equation

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)   ΔH = -802 kJ

<u>Step 2:</u> Given data

We notice that for 1 mole of methane (CH4), we need 2 moles of O2 to produce : 1 mole of CO2 and 2 moles of H20.

The enthalpy change of combustion, given here as  Δ H , tells us how much heat is either absorbed or released by the combustion of <u>one mole</u> of a substance.

In this case: we notice that the combustion of 1 mole of methane gives off (because of the negative number),  802.3 kJ  of heat.

<u>Step 3: </u>calculate the enthalpy change  for 3 moles

The -802 kj is the enthalpy change for 1 mole

The change in enthalpy for 3 moles = 3* -802 kJ = -2406 kJ

The change in enthalpy in the combustion of 3 moles of methane = -2406 kJ

5 0
3 years ago
A 25.0-mL sample of an H2SO4 solution requires 50.0 mL of 0.150 M NaOH to completely react with the H2SO4. What was the concentr
Nitella [24]
V( H₂SO₄) = 25.0 mL in liters = 25.0 / 1000 = 0.025 L
 M(H₂SO₄) = ?

V(NaOH) = 50.0 mL = 50.0 / 1000 = 0.05 L 
M(NaOH) = 0.150 M

number of moles NaOH :

n = M x V

n = 0.150 x <span> 0.05 
</span>
n = 0.0075 moles of NaOH 

H₂SO₄(aq) + 2 NaOH(aq) = Na₂SO₄(aq) + 2 H₂O(l)

1 mole H₂SO₄ ---------- 2 mole NaOH
? mole H₂SO₄ ---------- 0.0075 moles NaOH

moles = 0.0075 * 1 / 2

= 0.00375 moles of H₂SO₄

M(H₂SO₄) = n / V

M = 0.00375 / <span> 0.025

</span>= 0<span>.15 M
</span>
hope this helps!

8 0
3 years ago
Using your knowledge of reactions and mechanisms, draw the mechanism for the formation of 2-methylpropene from 2-methyl-2-propan
BARSIC [14]

Answer:

Here's what I get  

Explanation:

The reaction is an E1 elimination of an alcohol to form an alkene. It has three steps:

1. Protonation

The alcohol is protonated with aqueous sulfuric acid to convert it into a better leaving group.

2. Loss of the leaving group

A water molecule leaves in a unimolecular process to form a stable 3° carbocation.

3. Loss of an α-hydrogen

A water molecule removes an α-hydrogen, forming 2-methylpropene and regenerating the original hydronium ion.

4 0
3 years ago
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