All categories

3 years ago

Find the density of an object that has a mass of 5 kg and a volume of 50 cm3.

Chemistry

1 answer:

iren2701 [21]3 years ago

4 0

Mass=5kg=5000g
Volume=50cm^3

$\\ \rm\longmapsto Density=\dfrac{Mass}{Volume}$

$\\ \rm\longmapsto Density=\dfrac{5000}{50}$

$\\ \rm\longmapsto Density=100g/cm^3$

You might be interested in

A certain reaction at equilibrium has more moles of gaseous products than of gaseous reactants.(b) Write a statement about the r

mojhsa [17]

To be equal as $K_p$ , $K_c$ needs to be divided by $(RT)^{\Delta n}$

<h3>Briefly explained</h3>

When the amount of gaseous reactant is greater than the amount of gaseous product, where $n_{products} < n_{reactants}$ ,

then = $K_p < K_c$

It's because $\Delta n$ is negative, which places (RT) in the denominator. This is how the equation will now appear.

$K_p = K_c(RT)^{-\Delta n} = \frac{ K_c}{(RT)^{\Delta n}}$

Here you can observe the value of $K_c$ is greater than $K_p$ . To be equal as $K_p$ , $K_c$ needs to be divided by $(RT)^{\Delta n}$

<h3>What is Δngas?</h3>

The number of moles of gas that move from the reactant side to the product side is denoted by the symbol ∆n or delta n in this equation.

Once more, n represents the growth in the number of gaseous molecules the equilibrium equation can represent. When there are exactly the same number of gaseous molecules in the system, n = 0, Kp = Kc, and both equilibrium constants are dimensionless.

<h3>Definition of equilibrium</h3>

When a chemical reaction does not completely transform all reactants into products, equilibrium occurs. Many chemical processes eventually reach a state of balance or dynamic equilibrium where both reactants and products are present.

Learn more about equilibrium

brainly.com/question/11336012

#SPJ4

6 0

2 years ago

2. Circle the letter of each sentence that is true about numbers expressed in

ivanzaharov [21]

Answer:

I think it is b) NOT SURE

Explanation:

5 0

3 years ago

Which of the following has kinetic energy?

Maurinko [17]

Answer:

Explanation:

Movement

5 0

4 years ago

How many moles of potassium chloride and oxygen can be produced from 100.0g of potassium chlorate? The balanced equation is: 2 K

natka813 [3]

100.0 g KClO₃ × 1 mol KClO₃/122.55 g KClO₃ × 2 mols KCl/2 mols KClO₃= 0.8160 mols of KCl

100.0 g KClO₃ × 1 mol KClO₃/122.55 g KClO₃ × 3 mols O₂/ 2 mols KClO₃= 1.224 mols of O₂

try this

122.55 g is molar mass of potassium chlorate

4 0

3 years ago

Read 2 more answers

Why are the optimum conditions for the Haber process a temperature of 450°C and pressure of 200 atmospheres?

Novay_Z [31]

Answer:

See explanation.

Explanation:

Hello,

Haber process is defined as the widely acknowledged productive process of ammonia by the reaction:

$N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)$

Which is carried out in gaseous phase. Thus, by means of the Le Chatelier's principle, it is possible to know that its standard enthalpy of reaction is -45.90 kJ/mol (NIST webbook) for which it is an exothermic chemical reaction, for that reason less ammonia will be produced at high temperature, nonetheless, the temperature should not be too low since the reaction rate significantly decrease, therefore, the optimum found temperature is 450 °C.

Moreover, since there are more moles (3+1=4) at the reactants and less moles at the products (2), increasing the pressure of the reaction increases the yield of ammonia, nonetheless, higher pressures involve the purchasing of more expensive equipment to withstand the high-pressures, for that reason, the best found pressure has been set as 200 atm.

Best regards.

8 0

4 years ago

Read 2 more answers