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3 years ago

The picture explains it.

Chemistry

1 answer:

Rainbow [258]3 years ago

5 0

Answer:

E, and H

Explanation:

they are opinions, not facts

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What is covalent bond

katen-ka-za [31]

Covalent bonding is when electrons are shared between atoms.

7 0

3 years ago

Read 2 more answers

N2 +3H2 → 2NH3 What volume of ammonia at STP is produced if 30.0 g of nitrogen gas is reacted with an excess of hydrogen gas?

WARRIOR [948]

Answer:

V= 48L

Explanation:

Moles of N2 = m/M = 30/28= 1.07moles

From the equation of reaction

N2 +3H2 → 2NH3

1mole of N2 produces 2mole of NH3

Hence

1.07moles will produce 1.07×2= 2.14 moles

At STP, 1mole occupy 22.4L

Hence volume of N2 produced = 2.14×22.4= 48 L

3 0

4 years ago

Why ddo all collisions between reactant molecules not lead to reaction.

jok3333 [9.3K]

Answer:

The colliding molecules need to possess certain energy which is greater than the activation energy Ea and proper orientation.

<h3>Not all collisions result in a chemical reaction because not all collisions have the have sufficient amount of energy or have the appropriate activation energy. Nor do they all have this correct orientation. Molecules need to collide in such a way that they're oriented, so the correct bonds could break in. The correct bonds conform. And then, of course, they need to have sufficient activation energy in order to initiate the breaking of the bonds.</h3>

<h3>Hope this helps please let me know If I'm wrong.</h3>

7 0

2 years ago

Suppose that 98.0g of a non electrolyte is dissolved in 1.00kg of water. The freezing point of this solution is found to be -0.4

Sholpan [36]

Answer:

$\large \boxed{\text{392 u}}$

Explanation:

1. Calculate the molal concentration

The formula for the freezing point depression by a nonelectrolyte is

$\Delta T_{f} = -K_{f}b\\b = -\dfrac{\Delta T_{f}}{ K_{f}} = -\dfrac{-0.465 \, ^{\circ}\text{C}}{\text{1.86 $\, ^{\circ}$C$\cdot$kg$\cdot$mol}^{-1}} = \text{0.250 mol/kg}$

2. Calculate the moles of solute

$\begin{array}{rcl}b & = & \dfrac{\text{moles of solute}}{\text{kilograms of solvent}}\\\\\text{moles of solute} & = & b \times {\text{kilograms of solvent}}\\n & = &\text{0.250 mol/kg} \times \text{1.00 kg}\\ & = & \text{0.250 mol}\\\end{array}$

3. Calculate the molecular mass

$\begin{array}{rcl}\text{Moles} & = &\dfrac{\text{mass}}{\text{molar mass}}\\\\\text{0.250 mol} & = & \dfrac{\text{98.0 g}}{MM}\\\\MM & = & \dfrac{\text{98.0 g }}{\text{0.250 mol}}\\\\& = &\textbf{392 g/mol}\\\end{array}\\\text{The molecular mass of the solute is $\large \boxed{\textbf{392 u}}$}$

3 0

4 years ago

What is the mass of one mole of Ca(OH)2?

marshall27 [118]

Answer:

74.10g/mol

Explanation:

The mass of one mole of Ca(OH)₂ is the molar mass of the compound.

To solve this problem, we add the atomic masses of the species in the compound;

Atomic mass of Ca = 40.078g/mol

O = 15.9994g/mol

H = 1.0079g/mol

So;

Molar mass = 40.078 + 2(15.9994 +1.0079 ) = 74.10g/mol

3 0

3 years ago