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2 years ago

What is the main precaution to take if a gas cylinder sign is present in the lab? select one

1 answer:

4 0

The main precautions to take if a gas cylinder sign is present in the lab visually check that the gas cylinder is restrained, but keep a safe distance from it. The correct option is c.

<h3>What are the precautions?</h3>

Precautions are the preventive steps that are taken to save yourself from any dangerous circumstances. These steps are always taken in doing experiments and other scientific procedures.

Here, the precautions are to check the gas cylinder.

Thus, the correct option is c, Visually check that the gas cylinder is restrained, but keep a safe distance from it.

To learn more about precautions, refer to the link:

brainly.com/question/15622844

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The question is incomplete. Your most probably complete question is given below:

Remove the strap from around the gas cylinder to use it in the lab.

Open the valve on the gas cylinder periodically to release pressure.

Visually check that the gas cylinder is restrained, but keep a safe distance from it.

Test out the regulator on the gas cylinder to make sure it is working properly.

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Explain how you would expect the strength of

LekaFEV [45]

Answer:

You should expect that the ionic bond in LiBr is stronger than the bond in KBr.

Explanation:

The ionic bonds are formed by the electrostatic attraction between the ions, cations and anions.

In KBr the cation is K⁺ and the anion is Br⁻.

In LiBr the cation is Li⁺ and the anion is Br⁻.

You must expect that the bond strength depends mainly on the charges present on each ion and the distance between them.

Nevertheless, the effect of the distance between the radius dominate the trendency of the bond strength, which makes that the ionic strength trend be related to the ionic radius trend.

Lithium is a smaller ion than Potassium (both are in the same group and Lithium is above Potassium).

Thus, you should expect that the Li ion is closer to the Br ion than what the K ion is to the Br ion and expect that the bond between a Li ion and the Br ion be stronger than the bond between the K ion and the Br ion.

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3 years ago

Write the chemical formula of baking soda ?

Fantom [35]

Answer:

NaHCO₃

Explanation:

NaHCO₃ is the chemical formula for sodium bicarbonate or baking soda. It has one sodium atom, one hydrogen atom, one carbon atom, and three oxygen atoms.

Have a good day and stay safe!

6 0

4 years ago

Read 2 more answers

HELLPPPPPP!

lukranit [14]

Answer:

Because the melting of ice as a spontaneous process (or reaction).

Explanation:

Here is an example:

Take a ice on a plate and leave it for half an hour (conditions). After half an hour, we notice water instead of ice.

This process took place without any intervention from your side. Heat absorbed by the ice from surrounding is due to set of conditions not due to your intervention.

So, we can consider melting of ice as a spontaneous process (or reaction).

6 0

3 years ago

When 2 grams of Hydrogen (H2) react with 32 grams of Oxygen (O2) the reaction yields hydrogen peroxide (H2O2). How many grams of

Alisiya [41]

Given information:

Mass of H2 = 2 g

Mass of O2 = 32 g

To determine:

Mass of H2O2 produced

Explanation:

The reaction between H2 and O2 can be given as:

H2 + O2 → H2O2

Based on the reaction stoichiometry:

1 mole of H2 reacts with 1 mole of O2 to form 1 mole of H2O2

# moles of H2 = mass of H2 / molar mass of H2 = 2 g/ 2 g.mol-1 = 1 mole

# moles of O2 = mass of O2/ molar mass of O2 = 32 g/ 32 g.mol-1 = 1 mole

Hence for the given reactant conditions, moles of H2O2 produced = 1

Mass of H2O2 = moles of H2O2 * molar mass H2O2 = 1 mole * 34 g.mole-1 = 34 g

Ans: 34 g of H2O2 is produced in this reaction

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3 years ago

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You can measure how much of something you have by counting individual objects. For example, you can count the number of cookies

Artyom0805 [142]

Answer:

Explanation: first use a balance to get the masses of these items. Once the masses of these items are measured, we can then calculate the moles.

The mole is = mass/molarmass

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3 years ago