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VARVARA [1.3K]
3 years ago
7

I need hellppp please.

Chemistry
1 answer:
sasho [114]3 years ago
4 0
C3H8.gas reacts with 5L of O2 at STP
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Given the information shown in process "B", calculate the molar enthalphy of fusion for ice
Nikolay [14]

Answer:

D) 6.02 kJ/mol

Explanation:

Hello,

In this case, since 200kJ melted 1.5 kg of ice (2.0kg-0.5kg), we can compute the melted moles:

n=\frac{1.5kg}{18kg/kmol} *\frac{1000mol}{1kmol}=83.33mol

Then, we compute the molar enthalpy of fusion by diving the melted moles to the applied heat:

\Delta H_{fusion}=\frac{500kJ}{83.33mol}\\ \\\Delta H_{fusion}=6.02kJ/mol

Hence answer is D) 6.02 kJ/mol.

Best regards.

6 0
3 years ago
Help sdfghrthfbfdve aahhhhhhhh
nirvana33 [79]
I believe the answer is C !
5 0
2 years ago
Due Tomorrow!<br><br> What is [OH-] of a solution<br> with a pH of -1.0? <br><br> Answer in M
Margaret [11]
M IS A LETTER but N is a letter
8 0
3 years ago
Manganese forms several oxides when combined with oxygen. One of the oxides (Oxide 1) contains 63.2% of Mn and another oxide (Ox
Nina [5.8K]

Explanation:

Defining law of definite proportions, it states that when two elements form more than one compound, the ratios of the masses of the second element which combine with a fixed mass of the first element will always be ratios of small whole numbers.

A. One of the oxides (Oxide 1) contains 63.2% of Mn.

Mass of the oxide = 100g

Mass of Mn = 63.2 g

Mass of O = 100 - 63.2

= 36.8 g

Ratio of Mn to O = 63.2/36.8

= 1.72

Another oxide (Oxide 2) contains 77.5% Mn.

Mass of oxide = 100 g

Mass of Mn = 77.5 g

Mass of O = 100 - 77.5

= 22.5 g

Ratio of Mn to O = 77.5/22.5

= 3.44

Therefore, the ratio of the masses of Mn and O in Oxide 1 and Oxide 2 is in the ratio 1.72 : 3.44, which is also 1 : 2. So the law of multiple proportions is obeyed.

B.

Oxide 1

Mass of Mn per 1 g of O = mass of Mn/mass of O

= 77.5/22.5

= 3.44 g/g of Oxygen.

Oxide 2

Mass of Mn per 1 g of O = mass of Mn/mass of O

= 77.5/22.5

= 3.44 g/g of Oxygen.

3 0
3 years ago
The density of concentrated ammonia, which is 28.0% w/w nh3, is 0.899 g/ml. what volume of this reagent should be diluted to 1.0
vlada-n [284]

Answer: 2.4 ml

Solution :

Molar mass of NH_3 = 17 g/mole

Given,: 28% w/w of NH_3 solution means 28 g of ammonia in 100 g of solution.

Mass of solution = 100 g

Now we have to calculate the volume of solution.

Volume=\frac{Mass}{Density}=\frac{100g}{0.899g/ml}=111.2ml  

Molarity : It is defined as the number of moles of solute present in one liter of solution.

Molarity=\frac{n\times 1000}{V_s}

where,

n = moles of solute NH_3=\frac{\text {given mass}}{\text {molar mass}}=\frac{28}{17}=1.65moles

V_s = volume of solution in liter = 0.11 L

Now put all the given values in the formula of molarity, we get

Molarity=\frac{1.65moles}{0.11L}=15mole/L

Using molarity equation:

M_1V_1=M_2V_2

15\times V_1=0.036\times 1.0\times 10^{3}

V_1=2.4ml

6 0
3 years ago
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