Phosphorus burns in pure oxygen with a brilliant white light. The product of the combustion is...
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Phosphorus burns in pure oxygen with a brilliant white light. The product of the combustion is 43.64% phosphorus and 56.36% oxygen. What is the empirical formula of the product?
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PO2.5
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P2O5
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P2O3
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PO
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Homework Answers
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Phosphorus burns in pure oxygen with a brilliant white
light. The product of the combustion is...
When elemental phosphorus,P4 , burns in oxygen gas, it produces an intensely bright light, a great...
When elemental phosphorus,P4 , burns in oxygen gas, it produces an intensely bright light, a great deal of heat, and massive clouds of white, solid phosphorus(V) oxide (P2O5) product. Given these properties, it is not surprising that phosphorus has been used to manufacture incendiary bombs for warfare. Choose the unbalanced equation for the reaction of phosphorus with oxygen gas to produce phosphorus(V) oxide.
4.72 grams of pure phosphorus are allowed to react with oxygen in air to form an...
4.72 grams of pure phosphorus are allowed to react with oxygen in air to form an oxide. If the product weights 10.82 grams, find the empirical formula of the compound. Show all steps.
Please Help!!!!! A white powder is analyzed and found to contain 43.64% phosphorus and the rest...
Please Help!!!!!
A white powder is analyzed and found to contain 43.64% phosphorus and the rest oxygen by mass. The compound has a molecular weight of 283.88 g/mol. What are the compounds empirical and molecular formulas?
A compound of phosphorus and oxygen contains 43.64 % by mass phosphorous. The empirical formula is...
A compound of phosphorus and oxygen contains 43.64 % by mass phosphorous. The empirical formula is (a) PO (6) PO₂ (c) P₂0 (d) PO (1) P₃0. Assuming ideal gas behavior, the density, in g/L of N,O(g) at 1.53 atm and 45.2 °C is (b) 1.76 g/L (c) 16.4 g/L (a) 18.2 g/L (e) none of the above. (d) 2.58 g/L When the measured quantity 7.43 g/cm is converted to kg/m the answer is (a) 7.43 x10 kg/m² (b) 7.43 x...
Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.20 g of magnesium r...
Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.20 g of magnesium ribbon burns with 6.75 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation:_________________________ What is the limiting reactant? oxygen OR magnesium If the percent yield for the reaction is 79.9%, how many grams of product were recovered?...
Magnesium (Mg) combusts in air to give a brilliant white light that has been used in...
Magnesium (Mg) combusts in air to give a brilliant white light that has been used in photographic flashes and emergency flares. How much heat is produced if 10.0 g Mg is combusted with excess oxygen gas? Mg(s) + O2(g)-MgO(s) ard," =-601.6 kJ/mol Report your answer with three significant figures. . Provide your answer below: kJ
What is the empirical formula of a compound which contains only phosphorus and oxygen if a...
What is the empirical formula of a compound which contains only phosphorus and oxygen if a 4.19 gram sample of the compound contains 1.83 grams of oxygen and 2.36 grams of phosphorus? List the phosphorus first in your answer. You will not be able to type subscripts. Just type the numbers where they go. For example, S2O3 would be typed in as S2O3.
a sample of an unknown compound was analyzed and found to contain 19.97% phosphorus and oxygen....
a sample of an unknown compound was analyzed and found to contain 19.97% phosphorus and oxygen. What is the empirical formula of the compound? 4, Calculate the empirical formula for the compound formed when 10.83 g of zinc are heated with sulfur to form 16.16 g of zinc sulfide.
Pure magnesium metal is often found as ribbons and can easily burn in the presence of...
Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.29 g of magnesium ribbon burns with 7.42 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? O magnesium oxygen If the percent yield for the reaction is 90.7%, how many grams of product were recovered?...
2. Dimethylamine burns in oxygen according to the following equation: 4 C2H7N + 15 O2 →...
2. Dimethylamine burns in oxygen according to the following equation: 4 C2H7N + 15 O2 → 8 CO2 + 14 H2O + 2 N2 (a) How many liters of O2 at 35 °C and 0.840 atm will be needed to burn 7.70 L of C2H7N at 35 °C and 0.840 atm? (b) How many liters of CO2 at 35 °C and 0.840 atm will be produced? Report your answers to parts (a) and (b) to 3 significant figures. 3. Complete...
Please Help!!!!!
A white powder is analyzed and found to contain 43.64% phosphorus and the rest oxygen by mass. The compound has a molecular weight of 283.88 g/mol. What are the compounds empirical and molecular formulas?
A compound of phosphorus and oxygen contains 43.64 % by mass phosphorous. The empirical formula is (a) PO (6) PO₂ (c) P₂0 (d) PO (1) P₃0. Assuming ideal gas behavior, the density, in g/L of N,O(g) at 1.53 atm and 45.2 °C is (b) 1.76 g/L (c) 16.4 g/L (a) 18.2 g/L (e) none of the above. (d) 2.58 g/L When the measured quantity 7.43 g/cm is converted to kg/m the answer is (a) 7.43 x10 kg/m² (b) 7.43 x...
Magnesium (Mg) combusts in air to give a brilliant white light that has been used in photographic flashes and emergency flares. How much heat is produced if 10.0 g Mg is combusted with excess oxygen gas? Mg(s) + O2(g)-MgO(s) ard," =-601.6 kJ/mol Report your answer with three significant figures. . Provide your answer below: kJ
a sample of an unknown compound was analyzed and found to contain 19.97% phosphorus and oxygen. What is the empirical formula of the compound? 4, Calculate the empirical formula for the compound formed when 10.83 g of zinc are heated with sulfur to form 16.16 g of zinc sulfide.
Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.29 g of magnesium ribbon burns with 7.42 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? O magnesium oxygen If the percent yield for the reaction is 90.7%, how many grams of product were recovered?...
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