Questions and Answers
Given that the compound contains 1.20 grams of phosphorus for every 4.12 grams of chlorine, what is the weight ratio of phosphorus to chlorine?
The weight ratio of phosphorus to chlorine is 1.20:4.12.
If a sample of the compound has 6.22 grams of chlorine, how many grams of phosphorus are in that sample?
There are approximately 1.81 grams of phosphorus in the sample.
How can you set up a proportion to determine the amount of phosphorus in a sample containing 6.22 grams of chlorine?
Set up the proportion as $\frac{1.20}{4.12} = \frac{x}{6.22}$, where x is the grams of phosphorus.
What is the first step you would take to find the grams of phosphorus in the given sample of chlorine?
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What key concept from stoichiometry allows you to calculate the grams of phosphorus from the amount of chlorine present?
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Berapa banyak gram fosfor yang terkandung dalam 6,22 gram klorin, jika rasio fosfor dan klorin dalam senyawa adalah 1,20:4,12?
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Senyawa yang terdiri dari fosfor dan klorin memiliki berat yang sama antara keduanya.
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Jika senyawa mengandung 1,20 gram fosfor untuk setiap 4,12 gram klorin, berapa proporsi fosfor yang ada dalam 10 gram senyawa tersebut?
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Dalam rasio 1,20 gram fosfor untuk 4,12 gram klorin, fosfor adalah _____ dari total berat senyawa.
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Cocokkan rasio komponen pada senyawa dengan beratnya:
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Study Notes
Compound Composition
- The compound consists of phosphorus and chlorine in a specific mass ratio.
- The mass ratio: 1.20 grams of phosphorus per 4.12 grams of chlorine.
Calculation Based on Mass
- For every 1.20 g of phosphorus, there are 4.12 g of chlorine.
- To find the grams of phosphorus in a sample containing 6.22 g of chlorine, a proportion calculation is used.
Proportion Setup
- Establish the ratio:
- Phosphorus/Chlorine = 1.20 g P / 4.12 g Cl.
- Set up the equation to find phosphorus in a 6.22 g chlorine sample:
- Let x be the mass of phosphorus corresponding to 6.22 g of chlorine.
Solving for Phosphorus
- Use cross-multiplication to solve for x:
- ( \frac{1.20 g}{4.12 g} = \frac{x g}{6.22 g} )
Final Calculation
- Multiply and solve the proportion to find the grams of phosphorus in 6.22 g of chlorine.
- Result: The calculated mass of phosphorus will provide the required answer.
Application in Industry
- This compound is utilized in manufacturing flame retardant treatments for fabrics, emphasizing its practical significance.
Compound Composition
- The compound consists of phosphorus and chlorine in a specific mass ratio.
- The mass ratio: 1.20 grams of phosphorus per 4.12 grams of chlorine.
Calculation Based on Mass
- For every 1.20 g of phosphorus, there are 4.12 g of chlorine.
- To find the grams of phosphorus in a sample containing 6.22 g of chlorine, a proportion calculation is used.
Proportion Setup
- Establish the ratio:
- Phosphorus/Chlorine = 1.20 g P / 4.12 g Cl.
- Set up the equation to find phosphorus in a 6.22 g chlorine sample:
- Let x be the mass of phosphorus corresponding to 6.22 g of chlorine.
Solving for Phosphorus
- Use cross-multiplication to solve for x:
- ( \frac{1.20 g}{4.12 g} = \frac{x g}{6.22 g} )
Final Calculation
- Multiply and solve the proportion to find the grams of phosphorus in 6.22 g of chlorine.
- Result: The calculated mass of phosphorus will provide the required answer.
Application in Industry
- This compound is utilized in manufacturing flame retardant treatments for fabrics, emphasizing its practical significance.
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Description
This quiz explores the calculation of the mass of phosphorus in a compound based on its ratio with chlorine. Participants will use given quantities to determine the mass of phosphorus contained within a specified amount of chlorine. It's a practical application of stoichiometry in chemistry.
