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2 years ago

How many grams of nh3 can be produced from 3.80 mol of n2 and excess h2?

1 answer:

4 0

The balanced equation :N2 + 3H2 --> 2NH3

1) Let's find the molar mass of NH3 because it will be needed later.
To determine the molar mass you have to consult the periodic table and see the atomic mass of each element. If the element is repeted, for example 3 times, you multiple the atomic mass per 3.
NH3= 14 + 1 x 3= 17 g/mol

2) By looking at the balanced equation, you can see that 2 mol of NH₃ were produced with only one mol of N2. How much NH3 will result when we have 3,80 mol of N2?
So now we solve it with a porportion:

2 mol NH3-------1 mol of N2
x --------<span>3.80 of N2

x= 2 x3,8 = 7,6</span><span>mol NH3

3) </span> the only thing left to do is convert the moles obtained, to grams. We can use the formula:
nº of moles x molar mass= mass
7,6mol NH3 x 17 g/mol= mass of NH3
mass= 129,2 grams of NH3

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Constance has an apple that weighs 85,000 milligrams and a peach that weighs 0.15 kilograms. which fruit has the greater mass? c

Rama09 [41]

The fruit which has the greater mass is peach i.e. 150 grams.

Mass is a quantity which is used to define that what amount of substance will occupy any space or present in the given object.

We have given,

Weight of apples = 85,000 mg

Weight of peach = 0.15 kg

To compare the quantity first we have to convert both of these units in the same unit, and we know that:

In 1 kilogram = 1000 grams

And in 1 grams = 1000 milligrams

So, we convert both the units into grams as:

85,000 mg = 85,000 / 1000 = 85 grams

0.15 kg = 150 grams

So, the mass of peach is high.

Hence, peach has the greater mass.

To know more about mass, visit the below link:

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4 0

1 year ago

Consider the data presented below. time (s) 0 40 80 120 160 moles of a 0.100 0.067 0.045 0.030 0.020 part a part complete determ

Whitepunk [10]

To determine which order of the reaction it is, first we need to calculate the rate of change of moles.
the data is as follows
time 0 40 80 120 160
moles 0.100 0.067 0.045 0.030 0.020

Q1)
for the first 40 s change of moles ;
= -d[A] / t
= - (0.067-0.100)/40s
= 8.25 x 10⁻⁴ mol/s
for the next 40 s
= -(0.045-0.067)/40
= 5.5 x 10⁻⁴ mol/s
the 40 s after that
= -(0.030-0.045)/40 s
= 3.75 x 10⁻⁴ mol/s
k - rate constant
and A is the only reactant that affects the rate of the reaction

rate = k [A]ᵇ
8.25 × 10⁻⁴ mol/s = k [0.100 mol]ᵇ ----1
5.5 x 10⁻⁴ mol/s = k [0.067 mol]ᵇ -----2
divide the 2nd equation by the 1st equation
1.5 = [1.49]ᵇ
b is almost equal to 1
Therefore this is a first order reaction

Q2)
to find out the rate constant(k), we have to first state the equation for a first order reaction.
rate = k[A]ᵇ
As A is the only reactant thats considered for the rate equation.
Since this is a first order reaction,
b = 1
therefore the reaction is
rate = k[A]
substituting the values,
8.25 x 10⁻⁴ mol/s = k [0.100 mol]
k = 8.25 x 10⁻⁴ mol/s /0.100mol
= 8.25 x 10⁻³ s⁻¹

7 0

2 years ago

What is the name for NH

rjkz [21]

Answer:

Due to the lack of context for your question I’m not completely sure which you are talking about but NH can be Imidogen or it could be ammonium which is NH4^1+

4 0

2 years ago

8. What is the heat of reaction when hydrogen and oxygen combine to form water?

valina [46]

Answer:

The heat of reaction when hydrogen and oxygen combine to form water is :

Explanation:

Enthalpy Change = The enthalpy change for the formation of 1 mole of the substance from their standard state is called the enthalpy of formation.

This is intensive quantity as it is fixed for 1 mole .

Intensive properties = Those properties which are independent on the amount of the substance are intensive properties.

The value of these quantities does not get halve if you divide the substance into two equal parts. example , density, refractive index.

However , the enthalpy of reaction is extensive. Because on increasing the amount the value of the enthalpy also get doubles

Hence for this reaction :

$2H_{2}(g)+O_{2}\rightarrow 2H_{2}(l)$

Its value is -285.8 kJ for 1 mole

And here two moles are present . so the value of molar enthalpy is:

-285.8 x 2 = -571.6 kJ

8 0

3 years ago

(b) What amount (mol) of H₂ can be produced from the given mass of H₂O?

Luden [163]

8 moles of H 2O are produced.

First, we need to figure out the chemical equation for producing water with oxygen which is H 2 + O2 = H 2O. Then, we need to balance the equation, resulting in 2H 2 + O2 = 2H 2O.

<h3>How many moles of H2 are required to make one mole of NH3?</h3>

Calculate 0.88074 mol H2's mass. If N2 is too much, 1.776 g H2 is needed to create 10.00 g of NH3. To create 8.2 moles of ammonia, 2 moles of NH3 are created when 1 mole of N2 and 3 moles of H2 mix. 4.1 moles of N2 Fast are consequently needed to make 8.2 moles of NH3.

<h3>How many moles of h2 are needed to produce a solution?</h3>

An O-H bond has a bond energy of 1 09 Kcal. 3.6. A 38.0mL 0.026M HCl solution and a 0.032M NaOH solution react. Thus, 10 moles of NH 3 are obtained by dividing 15 moles of H2 by the 1.5 moles of H2 required for the product. and 9.3 x 10-3 moles of bromobutane (1.27/137 =.00927moles).

Learn more about H2O:

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#SPJ4

8 0

1 year ago