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neonofarm [45]
2 years ago
12

A volume of gas at 1.10 atm was measured at 507 ml. What will be the volume if the pressure is adjusted to 1.90

Chemistry
1 answer:
Ksivusya [100]2 years ago
3 0

Answer:

294mL

Explanation:

We can use this equation to find the unknown volume:

P_1V_1=P_2V_2

To solve, plug in the values we have and solve for the unknown value:

(1.10atm)(507mL)=(1.90atm)V_2\\\frac{(1.10atm)(507mL)}{1.90atm} =V_2\\V_2=293.53mL

Rounding to three significant figures gives you the value of 294mL

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Which option identifies all the bonds broken during this chemical reaction?
Tresset [83]

Answer:

the bond b/w oxygen and hydrogen atom

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2 years ago
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The volume of a pond being studied for the effects of acid rain is 35 kiloliters (kL). There are 1,000 liters (L) in 1 kL and 1
MrMuchimi
The volume of a pond being studied for the effects of acid rain is 35 kiloliters (kL). There are 1,000 liters (L) in 1 kL and 1 x 10^6 <span>microliters (mL) in 1 L. 

35 kL (1,000 L/ 1kL) (</span>1 x 10^6 microliters / 1 L) = 3.5 x 10^10 microliters<span>

The volume of this pond in microliters is </span><span>3.5 x 10^10 microliters</span>
8 0
3 years ago
2, 3-diethyl–4-octene  what is structure of this pls help​
pantera1 [17]

Answer:

(CH2CH3).

!

CH-CH-CH-CH=CH-CH2-CH2-CH3

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(CH2CH3)

2, 3-diethyl–4-octene

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4 0
3 years ago
5. Hydrogen &amp; oxygen react chemically to form water. How much water
stepladder [879]

39.25 g of water (H₂O)

Explanation:

We have the following chemical reaction:

2 H₂ + O₂ → 2 H₂O

Now we calculate the number of moles of each reactant:

number of moles = mass / molar weight

number of moles of H₂ = 14.8 / 2 = 7.4 moles

number of moles of O₂ = 34.8 / 32 = 1.09 moles

We see from the chemical reaction that 2 moles of H₂ will react with 1 mole of O₂ so 7.4 moles of H₂ will react with 3.7 moles of O₂ but we only have 1.09 moles of O₂ available. The O₂ will be the limiting reactant. Knowing this we devise the following reasoning:

if        1 moles of O₂ produces 2 moles of H₂O

then  1.09 moles of O₂ produces X moles of H₂O

X = (1.09 × 2) / 1 = 2.18 moles of H₂O

mass = number of moles × molar weight

mass of H₂O = 2.18 × 18 = 39.25 g

Learn more about:

limiting reactant

brainly.com/question/7144022

brainly.com/question/6820284

#learnwithBrainly

6 0
3 years ago
Calculate the feed ratio of adipic acid and hexamethylene diamine that should be employed to obtain a polyamide of approximately
artcher [175]

Answer:

r= 0.9949 (For 15,000)

r=0.995 (For 19,000)

Explanation:

We know that

Molecular weight of hexamethylene diamine = 116.21 g/mol

Molecular weight of adipic acid = 146.14 g/mol

Molecular weight of water = 18.016 g/mol

As we know that when  adipic acid  and hexamethylene diamine react then nylon 6, 6 comes out as the final product and release 2 molecule of water.

So

M_{repeat}=146.14+166.21-2\times 18.106\ g/mol

M_{repeat}=226.32\ g/mol

So

Mo= 226.32/2 =113.16 g/mol

M_n=X_nM_o

Given that

Mn= 15,000 g/mol

So

15,000 = Xn x 113.16

Xn = 132.55

Now by using Carothers equation we know that

X_n=\dfrac{1+r}{1+r-2rp}

132.55=\dfrac{1+r}{1+r-2\times 0.99r}

By calculating we get

r= 0.9949

For 19,000

19,000 = Xn x 113.16

Xn = 167.99

By calculating in same process given above we get

r=0.995

3 0
3 years ago
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