Craters visible on the moon's surface provide further evidence of

Which of the following series of scientific steps is most likely in the correct order?

Leni [432]

Observation, hypothesis, experiment is the correct answer

4 0

3 years ago

Read 2 more answers

Convert 7.1x10^25 molecules of water to moles

ruslelena [56]

Answer:

<h2>117.94 moles</h2>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

$n = \frac{N}{L} \\$

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

$n = \frac{7.1 \times {10}^{25} }{6.02 \times {10}^{23} } \\ = 117.940199...$

We have the final answer as

<h3>117.94 moles</h3>

Hope this helps you

8 0

3 years ago

We add a 1.20-g sample of dry ice to a 755-mL flask containing nitrogen gas at a temperature of 25.0 C and a pressure of 725mmHg

yaroslaw [1]

Answer:

Total pressure is 1396 mmHg

Explanation:

By:

PV/RT = n

It is possible to obtain the initial moles of nitrogen gas, where:

P is pressure (725 mmHg = 0,954 atm)

V is volume (0,755L)

R is gas constant (0,082atmL/molK)

T is temperature (25,0°C = 298,15 K)

Replacing:

n = 0,02946 moles of nitrogen gas.

The moles of dry ice (CO₂; molar mass= 44,01 g/mol) are:

1,20 g × (1mol/44,01g) = 0,02727 moles of dry ice.

When dry ice sublimes, total moles are:

0,02727 + 0,02946 =<em> 0,05673 moles</em>

With the temperature (25,0°C = 298,15 K) and volume (0,755L) it is possible to obtain total pressure, thus:

P = nRT/V

Replacing:

P = 1,837 atm × (760 mmHg/1atm) = <em>1396 mmHg</em>

I hope it helps!

3 0

3 years ago

Given the following equation,, how many moles of water will be produced when 12 moles of ethane (C2H6) are burned?

VARVARA [1.3K]

Answer: 36 mol H2O (l)

Explanation:

Let's use stoichiometry to solve this problem.

12 mol C2H6 * (6 mol H2O / 2 mol C2H6) = 36 mol H2O

Hope this helps!

6 0

3 years ago

Consider this reaction: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O, 18.6 moles of CO2, and

alisha [4.7K]

H₂O would be the limiting reactant.

Balanced chemical equation:

6CO₂ + 6H₂O + light equation → C₆H₁₂O₆ + 6O₂

The amount of product that can be created is constrained by the reactant that is consumed first in a chemical reaction, commonly referred to as the limiting reactant (or limiting reagent).

Given

No. of moles of CO₂ = 18.6

Mass of H₂O = 2.38 × 10² g = 238g

No. of moles of H₂O = Given mass/ Molar mass

= 238 / 18 = 13.22 moles

Moles of H₂O = 13.22

According to the balanced chemical equation

6 moles of CO₂ react with 6 moles of H₂O

So the reactant that has less number of moles will be consumed first.

As the No. of moles of H₂O < No. of moles of CO₂

So, H₂O is the limiting reactant with 13.22 moles.

Hence, H₂O would be the limiting reactant.

Learn more about limiting reactant here brainly.com/question/14222359

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7 0

2 years ago