What is the difference between an internal combustion engine and the diesel engine

Consider the chemical reaction: 2 cu(no3)2â†’ 2 cuo (s) + 4 no2 (g) + o2 (g)when 9.378 g of cu(no3)2 completely decomposed, how

Allushta [10]

2Cu(NO3)2 ----------> 2CuO (s) +4NO2 (g) + O2(g)

9.378g=0.05moles

no of moles = weight / MW = 9.378/187.56 = 0.05moles

as per the above reaaction 2moles of Cu(NO3)2 can produce 4moles of N2

0.05moles Cu(NO3)2 can produce (0.05*4)/2 = 0.1moles of N2

and 2moles of Cu(NO3)2 can produce 1moles of O2

0.05moles Cu(NO3)2 can produce (0.05*1)/2 = 0.025moles of O2

Total moles of gas i.e., N2 and O2 =0.1+0.025 = 0.125moles

From PV = nRT

V = nRT/ P = 0.125*0.0821*273 = 2.80166Lit option is correct

6 0

2 years ago

Elemental analysis of the unknown gas from part a revealed that it is 30.45% n and 69.55% o. what is the molecular formula for t

Gnesinka [82]

Assuming we have 100 g of sample

30.45/MW of N 14g = 2.175

69.55/MW of O 16g = 4.34

4.34/2.185 = 2

for every 1 mole of N we have 2 moles of O

so the empirical formula would be NO2

without having the molecular weight of the entire molecule the molecular formula can not be determined with the information in your question

6 0

2 years ago

Which statement Is true of chloroplasts? A. They transport glucose into the cell. B. They convert light energy into chemical ene

Lostsunrise [7]

answer is B. And chloroplast is only found is plant cells.

6 0

2 years ago

Read 2 more answers

112 g of aluminum carbide react with 174 g water to produce methane and aluminum hydroxide in the reaction shown below.

dolphi86 [110]

<u>Answer:</u> 4.999 moles of excess reactant will be left over.

<u>Explanation:</u>

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of aluminium carbide = 112 g

Molar mass of aluminium carbide = 143.96 g/mol

Putting values in equation 1:

$\text{Moles of aluminium carbide}=\frac{112g}{143.96g/mol}=0.778mol$

For the given chemical reaction:

$2Al_4C_3(s)+12H_2O(l)\rightarrow 3CH_4(g)+4Al(OH)_3(s)$

By the stoichiometry of the reaction:

2 moles of aluminium carbide reacts with 12 moles of water

So, 0.778 moles of aluminium carbide will react with = $\frac{12}{2}\times 0.778=4.668 mol$ of water

Given mass of water = 174 g

Molar mass of water = 18 g/mol

Putting values in equation 1:

$\text{Moles of water}=\frac{174g}{18g/mol}=9.667mol$

Moles of excess reactant (water) left = 9.667 - 4.668 = 4.999 moles

Hence, 4.999 moles of excess reactant will be left over.

8 0

2 years ago

PLEASEEE HELPPP I SUCK AT CHEM :(

Luda [366]

Answer:

a) H2SO4 + 2KOH -> 2H2O + K2SO4

b) 9.809 ml

Explanation:

Number of Moles = Mass/ Molar Mass

Therefore: Mass = Number of moles * Molar Mass

--------------------------------------------

Molar mass of H2SO4:

H2= 2.02

S= 32.07

O4= 64

--------------------------------------------

H2SO4 has the molar mass of 98.09

--------------------------------------------

the Moles of H2SO4 is given to be 0.100M

Therefore:

Mass= 98.09*0.1

= 9.809g

---------------------------------------------------

Assuming that 1 g= 1 ml, the volume of sulfuric acid is 9.809 ml.

7 0

2 years ago